A phosphoric acid (H3PO4) solution is 14.8 M with a density of 1.71 g/mL.
a) Determine the molality of the solution.
b) Determine the percent by mass of H3PO4 in the solution.

A) The molecular formula is: P₄O₁₀; B) This gives us the empirical formula: C₂H₆O

The simplest whole number ratio of atoms in a compound is called the empirical formula.

A) Empirical formula mass of P₂O₅ = 2(atomic mass of P) + 5(atomic mass of O)

= 2(30.97 g/mol) + 5(15.99 g/mol)

= 141.94 g/mol

Molecular mass / Empirical formula mass = 283.88 g/mol / 141.94 g/mol = 2

This tells us that the molecular formula is twice the empirical formula, so the molecular formula is: P₄O₁₀

B)  moles of C = 52.14 g / 12.01 g/mol = 4.344 mol

moles of H = 13.12 g / 1.01 g/mol = 12.97 mol

moles of O = 34.73 g / 16.00 g/mol = 2.17 mol

4.344 mol / 2.17 mol = 2.00

12.97 mol / 2.17 mol = 6.00

2.17 mol / 2.17 mol = 1.00

This gives us the empirical formula: C₂H₆O

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It took Approximately 52 minutes and 40 seconds for an electromagnetic signal to travel to Earth from Pioneer 11 when it was near Jupiter.

The speed of light, which is the speed at which an electromagnetic signal travels in a vacuum, is approximately 299,792,458 meters per second.

To find out how long it takes for an electromagnetic signal to travel from Pioneer 11 to Earth when it was near Jupiter, we can use the formula:

The distance between Pioneer 11 and Earth when it was near Jupiter is approximately 998 million km, or 998,000,000 km.

Converting this distance to meters, we get:

Dividing the distance by the speed of light, we get:

Converting this time to minutes and seconds, we get:

Rounding to the nearest minute and second, we get:

Therefore, it took approximately 52 minutes and 40 seconds for an electromagnetic signal to travel from Pioneer 11 to Earth when it was near Jupiter.

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Explanation:

Ideal gas law

PV = n R T        If P and V increase then T must increase

   ( n  and R   are constant)

Sugar cane plantation owners needed cheap labor after the enslaved were freed.

We know that in the nineteenth century the era of slave trade was actually coming to a close and the concern of many of the slave owners both in Europe and America was the future of their agricultural businesses.

The slave owners mostly used the slaves to do the work on the farm and in the absence of the slaves, the work could not be done. This is why the owners of the slaves sought for cheap labor after the slaves were freed.

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Sugar was important in the late nineteenth century for both dietary and economic reasons. It was consumed by all social classes and significantly influenced the labor practices in agriculture.

Based on the information provided, one can infer that sugar was of significant importance in the late nineteenth century. It served as a staple in people's daily diets and was enjoyed by all social classes, from shopgirls to kings. In the economic sphere, sugar cane farming was a notable industry. Sugar canes were labor-intensive to grow and harvest, which required plantation owners to seek cheap labor. This implies that the sugar industry had a substantial influence on labor practices during this era. It is therefore clear that sugar was not only a dietary necessity but also a crucial factor in the broader economic and social structure of the community.

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There are approximately 3.59 x [tex]10^{25}[/tex] molecules of [tex]CO_{2}[/tex] in 59.7 moles of [tex]CO_{2}[/tex].

What is Molecules?

Molecules are the smallest units of a chemical compound that retain the chemical properties and characteristics of that compound. They are composed of two or more atoms chemically bonded together. Molecules can be made up of atoms of the same element (as in diatomic molecules like oxygen gas, [tex]O_{2}[/tex]) or different elements (as in water,[tex]H_{2}O[/tex]which consists of two hydrogen atoms and one oxygen atom).

The term "59.7 molecules of [tex]CO_{2}[/tex]" is not a meaningful unit, as molecules are discrete entities and cannot be divided into fractions. However, assuming you meant to ask for the number of molecules in 59.7 moles of [tex]CO_{2}[/tex], we can use Avogadro's number to calculate it.

Avogadro's number is approximately 6.022 x [tex]10^{23}[/tex]molecules/mol, and it represents the number of entities (such as atoms, ions, or molecules) in one mole of a substance.

Given that you have 59.7 moles of [tex]CO_{2}[/tex], we can multiply this value by Avogadro's number to obtain the total number of molecules:

59.7 moles [tex]CO_{2}[/tex] x 6.022 x [tex]10^{23}[/tex] molecules/mol ≈ 3.59 x [tex]10^{25}[/tex] molecules of [tex]CO_{2}[/tex]

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a) Moles of HCI that were needed is 14.88 mol  ; b) Grams of HCI that were needed is 670.14 g.

Equation where number of atoms of each element in the reactant is equal to the number of atoms of the same element in the products is called as the balanced equation.

a.) 30 g / 2.016 g/mol = 14.88 mol of H₂

From the balanced equation, we can see that one mole of H₂ is produced for every mole of HCl consumed. Therefore, the number of moles of HCl needed is also 14.88 mol.

b.) 2 moles of HCl are consumed for every mole of PbCl₂ produced

So, the number of moles of HCl needed to produce 9.2 moles of PbCl₂ is:

9.2 mol PbCl₂ × 2 mol HCl/mol PbCl₂ = 18.4 mol HCl

18.4 mol × 36.46 g/mol = 670.14 g of HCl

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Several factors can dictate entropy in an equation.

These include:

1. Phase changes

⇒ When a solid turns to a liquid, the entropy increases as the particles have more freedom to move around and thus have a greater ability for 'disorder'. Same goes for a liquid turning to a gas. In a gas, the intermolecular forces are much weaker than that of a solid or liquid, allowing the particles more freedom.

So, going from a solid to liquid to gas increases entropy, and going the other way, from gas to liquid to solid, decreases entropy.

Example:

H₂O(l) -> H₂O(g)

This will have a positive entropy change, as the water molecules are becoming gaseous and thus have more freedom.

2. Dissolution

⇒ Similarly, breaking up particles of a solute when dissolving in a solvent will increase entropy as the particles are no longer bound together.

So, dissolving a solute will increase entropy.

Example:

NaCl(s) -> NaCl(aq)

This will have a positive entropy change, as the NaCl particles are more free after being separated.

3. Number of products and reactants

⇒ Generally, if you have more moles of products than reactants, if they are the same phase then entropy will increase. Note this is not necessarily true if you form a gas from two non-gas reactants, as the gas will still have more entropy.

4. Temperature

⇒ Increasing temperature will increase entropy as the particles have more kinetic energy and are then moving faster.

-------------------------------------------

l. 2N2(g) + O2(g) → 2N2O(g)

3 moles of gas are forming 2 moles of gas. The phase of products and reactants are the same, so since we have less moles of product than reactant, entropy will be negative.

II. CaCO3(s) → CaO(s) + CO2(g)

1 mole of solid is forming 1 mole of solid and 1 mole of gas. There is a phase change from solid to gas, and there are more moles of product than reactant, entropy will be positive.

III. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)​

While 3 moles of reactant are forming only 2 moles product, we are forming a gas from non-gaseous reactants, so entropy will be positive regardless.

The moles of carbon, hydrogen, and oxygen may not be whole numbers, we may need to round them to the nearest whole number to get the simplest ratio.

What is Empirical Formula?

The empirical formula of a chemical compound represents the simplest, most reduced ratio of atoms in that compound. It shows the relative number of atoms of each element present in the compound, expressed as the smallest whole numbers. In other words, it gives the simplest whole number ratio of the elements in a compound.

Mass of carbon = moles of CO

Mass of hydrogen = 2 x moles of H2O (since each H2O molecule has 2 hydrogen atoms)

Calculate the moles of oxygen in the compound.

Given:

Mass of oxygen = moles of CO (since each CO molecule has 1 oxygen atom) + moles of H2O (since each H2O molecule has 1 oxygen atom)

Determine the empirical formula.

The empirical formula represents the simplest, most reduced ratio of atoms in the compound. To determine it, we can use the mole ratios of carbon, hydrogen, and oxygen calculated in the previous steps.

Empirical formula = CxHyOz, where x, y, and z represent the mole ratios of carbon, hydrogen, and oxygen, respectively.

Now, let's plug in the calculated values for moles of carbon, hydrogen, and oxygen into the empirical formula:

Empirical formula = C moles : H moles : O moles

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The empirical formula of the unknown compound given the combustion analysis data is C2H3O.

The first step in solving this problem is to know how much carbon and hydrogen in grams are in the carbon dioxide (CO2) and water (H2O) produced. From the mass of CO2, we get 2.224g * 0.2729 (proportion of carbon in CO2) = 0.607g C. And the mass of hydrogen is 0.3035 g * 0.1119 (proportion of hydrogen in H2O) = 0.034g H. The remaining mass is 1g (total mass) - 0.607g C - 0.034g H = 0.359g O. Then, we need to convert these values to moles. This gives us 0.607g C * (1 mole C / 12.01 g C) = 0.050 moles C, 0.034g H * (1 mole H / 1.01 g H) = 0.033 moles H, and 0.359g O * (1 mole O / 16.00 g O) = 0.022 moles O.

By finding the ratio of these moles, we get C2H3O, which is the empirical formula of the compound.

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Given the following standard enthalpies of formation for the following substances, H2O (g) = -241.8 kJ/mol KOH (aq)=-482.4 kJ/mol KOH(s) =-425.8 kJ/mol The enthalpy of the reaction is -390.2 kJ/mol.

The standard enthalpy of formation, also known as the standard heat of formation, is the change in enthalpy that occurs during the synthesis of one mole of a substance from its component parts in their reference states, with all substances in their standard states. The IUPAC recommends using the standard pressure value of p = 105 Pa (= 100 kPa = 1 bar), while previous to 1982, the value of 1.00 atm (101.325 kPa) was used.A standard temperature doesn't exist. Its designation is fH. This symbol's superscript Plimsoll denotes that the process has been carried out under typical circumstances at the given temperature (typically 25 °C or 298.15 K).

The enthalpy of the reaction can be calculated using Hess's Law and the standard enthalpies of formation for the reactants and products. First, we need to determine the enthalpy of the reaction, ∆Hrxn. This is the sum of the standard enthalpies of formation for the products minus the sum of the standard enthalpies of formation for the reactants.

∆Hrxn = [2(-482.4) kJ/mol + (-241.8) kJ/mol] - [2(-425.8) kJ/mol + (-285.8) kJ/mol]

∆Hrxn = -390.2 kJ/mol

Therefore, the enthalpy of the reaction is -390.2 kJ/mol.

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The concentration of NaOH in the resulting solution is 1.80 mol/L.To determine the concentration of NaOH in the resulting solution, we need to use the equation:

What is concentration ?

concentration (in units of mol/L) = moles of solute / volume of solution (in units of L)

First, we need to calculate the moles of NaOH added to the flask:

moles of NaOH = mass of NaOH / molar mass of NaOH

moles of NaOH = 36.0 g / 40.00 g/mol

moles of NaOH = 0.900 mol

Next, we need to determine the volume of the solution. We know that 36.0 g of NaOH were added to a 500.0 mL volumetric flask, but the final volume of the solution is not given. We can assume that the volume of the solution is 500.0 mL, since that is the volume of the flask. However, we also need to take into account the fact that the addition of NaOH may cause the volume of the solution to increase slightly due to the dissolution of the solute.

Assuming that the volume of the solution is 500.0 mL, we can convert this to units of liters:

volume of solution = 500.0 mL / 1000 mL/L

volume of solution = 0.500 L

Now we can use the equation above to calculate the concentration of NaOH in the resulting solution:

concentration = 0.900 mol / 0.500 L

concentration = 1.80 mol/L

Therefore, the concentration of NaOH in the resulting solution is 1.80 mol/L.

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Complete question is: If 36.0 g of NaOH (MM = 40.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, 1.80 mol/L concentration of NaOH in the resulting solution.

Answer:

The balanced chemical equation for the combustion of C2H4 (ethylene) is:

C2H4 + 3 O2 → 2 CO2 + 2 H2O

From the balanced chemical equation, we can see that 1 mole of C2H4 reacts to produce 2 moles of H2O.

First, we need to convert the given mass of C2H4 to moles using its molar mass. The molar mass of C2H4 is:

2(12.01 g/mol) + 4(1.01 g/mol) = 28.05 g/mol

Now, we can calculate the moles of C2H4:

moles of C2H4 = mass of C2H4 / molar mass of C2H4

moles of C2H4 = 16 g / 28.05 g/mol

moles of C2H4 ≈ 0.570 mol (rounded to three decimal places)

According to the balanced chemical equation, 1 mole of C2H4 produces 2 moles of H2O.

moles of H2O = 2 * moles of C2H4

moles of H2O = 2 * 0.570 mol

moles of H2O ≈ 1.140 mol (rounded to three decimal places)

Finally, we can convert the moles of H2O to grams using the molar mass of water (H2O), which is 18.015 g/mol.

mass of H2O = moles of H2O * molar mass of H2O

mass of H2O = 1.140 mol * 18.015 g/mol

mass of H2O ≈ 20.53 g (rounded to two decimal places)

So, approximately 20.53 grams of H2O will be produced by the combustion of 16 grams of C2H4.

Answer:  C1V1=C2V2

Explanation: i hope this help im want to help you please

leave 5

The combined gas law, which links a gas's pressure, volume, and temperature, can be used to solve this issue. When the balloon reaches an altitude with a pressure of 0.65 atm and a temperature of -150 C, its capacity will fall to 4.9 L.

The Centigrade scale, Celsius size, and Kelvin scale are the three scales that are most frequently used to measure temperature.Any item contains molecules that move or vibrate. Its temperature will rise when it is heated because the molecules are moving more quickly.A tool called a thermometer is used to measure it. the three units used to measure temperature.

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Enthalpy of the reaction of the following equation is the same as the enthalpy of formation. 2 Fe (s) + 3 Cla (g) → 2 FeCl (s).

The difference between total reactant and total product molar enthalpies, computed for substances in their standard states, is the standard enthalpy of reaction for a chemical reaction. As long as the enthalpy of mixing is taken into consideration as well, this can then be used to forecast the total chemical bond energy liberated or bound during reaction.

A reaction's standard enthalpy is defined so that it solely depends on the conditions that are prescribed for it, rather than just on the actual circumstances in which reactions take place. The two main circumstances in which thermochemical measurements are actually performed.

The change in enthalpy during the synthesis of 1 mole of a compound from its component elements in their reference state, with all substances in their standard states, is known as the standard enthalpy of formation or standard heat of formation of a compound. The IUPAC recommends using the standard pressure value of 105 Pa (100 kPa = 1 bar), while previous to 1982, the value of 1 atm (101.325 kPa) was used.

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The balanced equation for the given redox reaction in basic solution is:

NO2^- + Fe3+ + H2O → NO3^- + Fe2+ + OH^-

Here, NO2^- is oxidized to NO3^-, which means it loses electrons and undergoes an oxidation reaction. Fe3+ is reduced to Fe2+, which means it gains electrons and undergoes a reduction reaction.

To balance the equation in basic solution, we first balance the atoms that are not hydrogen or oxygen. We start with the Fe3+ ion, which is reduced to Fe2+. To balance the iron atoms, we add one electron to the left side of the equation:

Fe3+ + e^- → Fe2+

Next, we balance the nitrogen and oxygen atoms in NO2^- and NO3^- by adding H2O and OH^- to the appropriate sides of the equation:

NO2^- + H2O → NO3^- + OH^-

Finally, we balance the electrons by multiplying the Fe3+ reduction half-reaction by 2, and adding it to the oxidation half-reaction for NO2^-:

2Fe3+ + 2e^- → 2Fe2+

NO2^- + 2Fe3+ + 2H2O → NO3^- + 2Fe2+ + 2OH^-

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To produce 22.4 L of O2 at STP, we need 2 moles of H2O.

Standard temperature and pressure (STP) is a set of reference conditions used in chemistry and physics. It is defined as a temperature of 0 degrees Celsius (273.15 Kelvin) and a pressure of 1 atmosphere (760 mmHg or 101.3 kPa). At STP, 1 mole of any ideal gas occupies a volume of 22.4 liters.

The balanced chemical equation is :

2H2O(l) → 2H2(g) + O2(g)

From the equation, we can see that for every 2 moles of H2O, 1 mole of O2 is produced.

At STP (standard temperature and pressure), 1 mole of any ideal gas occupies 22.4 L.

Therefore, to produce 22.4 L of O2 at STP, we need 2 moles of H2O.

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Answer:A. The gas particles have essentially zero volume and no attraction

for one another.

Explanation:

Methamphetamine is an amphetamine that stimulates the central nervous system (CNS).

Methamphetamine works by facilitating the release of catecholamines from brain nerve terminals, including noradrenaline, dopamine, and serotonin, as well as by inhibiting their uptake. As a result, the concentration of these neurotransmitters in the synaptic cleft rises, stimulating postsynaptic receptors more intensely.

The catalytic reduction of 1-phenyl-2-propanone (P-2-P, benzyl methyl ketone, BMK, or phenylacetone) in the presence of ammonia or methylamine is the fundamental reaction in all processes used to create methamphetamine. The Leuckart method (non-metallic reduction) and catalytic metal reduction are currently the most widely used reduction techniques.

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Answer: 34.24 g

Explanation: The molar mass of CO(NH2) can be calculated by including up the nuclear masses of each component within the atom. The nuclear masses of carbon (C), oxygen (O), nitrogen (N), and hydrogen (H) are 12.01 g/mol, 16.00 g/mol, 14.01 g/mol, and 1.01 g/mol, individually.

Molar mass of CO(NH2) = 1 x molar mass of C + 1 x molar mass of O + 2 x molar mass of N + 4 x molar mass of H

Molar mass of CO(NH2) = 1 x 12.01 g/mol + 1 x 16.00 g/mol + 2 x 14.01 g/mol + 4 x 1.01 g/mol

Molar mass of CO(NH2) = 60.06 g/mol

Presently, we will utilize this molar mass to change over moles of CO(NH2) to grams of CO(NH2):

mass of CO(NH2) = number of moles x molar mass

mass of CO(NH2) = 0.57 mol x 60.06 g/mol

mass of CO(NH2) = 34.24 g

Hence, there are 34.24 grams of CO(NH2) in 0.57 moles of CO(NH2). The answer isn't among the choices, so we have to be calculate the proper reply.

To discover the proper reply, ready to utilize the relationship between moles and mass:

mass = moles x molar mass

mass = 0.57 moles x 60.06 g/mol = 34.24 g

Answer:

The student who models the sun should stand somewhere in the room between Earth and the stars. The exact location will depend on how the students have chosen to set up the model and the relative distances they have assigned to each object. However, a common location for the sun model in this type of model is near one of the walls of the room, at a distance that is proportionally farther away from Earth than the stars. This is because the sun is much larger than any other object in our solar system and is located at the center of it, while the stars are much farther away. The student who models the sun should also be holding a flashlight, as the sun is a source of light and heat for our planet and the other planets in our solar system.

Answer: very close to Earth.

Explanation: I took the test the 2nd answer" to Question

The sun releases a huge amount of energy.

About what fraction of this energy reaches Earth? "

is :

one-billionth

The word equation for the given skeleton equation is: Solid aluminum + gaseous oxygen → Solid aluminum oxide.

Chemical equations are a way of representing chemical reactions using chemical formulas and symbols. They provide a concise and standardized way of describing chemical reactions and are an important tool for chemists to communicate and understand chemical changes.

In any chemical equation, reactants are written on left side of an arrow, whereas the products are written on right side. The arrow indicates the direction of reaction, from the reactants to products.

Chemical equations use chemical formulas to represent the elements and compounds involved in a reaction.

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The magnetic quantum number (ml) represents the orientation of the orbital in three-dimensional space the only possible value of the magnetic quantum number ml for a 1s electron is 0.

Quantum is the smallest possible unit of a physical quantity, such as energy or momentum. It is a fundamental concept in quantum mechanics, which is the branch of physics that deals with the behavior of matter and energy at the atomic and subatomic level.

The idea of quantization was first proposed by Max Planck in 1900, when he discovered that energy is emitted and absorbed in discrete units called "quanta" when studying the behavior of light and blackbody radiation. Later, this idea was extended to other physical quantities, such as the momentum and position of particles.

According to quantum mechanics, the behavior of particles and systems cannot be fully described using classical mechanics, which assumes that particles have definite positions and velocities at all times. Instead, the behavior of particles and systems is described using wave functions, which represent the probability of finding a particle at a given position and time.

The principles of quantum mechanics have important applications in many areas of physics, including atomic and molecular physics, condensed matter physics, and particle physics. They are also the basis.

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Answer:

a. SOLUTION:

Step 1: Write the balanced chemical equation.

C₂H₄ + 3O₂ → 2CO₂ + 2H₂O

Step 2: Calculate the number of moles of CO₂ formed by each reactant.

• Using C₂H₄

Based on the balanced chemical equation, 1 mole of C₂H₄ is stoichiometrically equivalent to 2 moles of CO₂.

The molar mass of C₂H₄ is 28.054 g/mol.

• Using O₂

Based on the balanced chemical equation, 3 moles of O₂ is stoichiometrically equivalent to 2 mole of CO₂.

The molar mass of O₂ is 31.998 g/mol.

Step 3: Determine the limiting reagent.

Since O₂ produced less amount of CO₂ than C₂H₄, O₂ is the limiting reagent.

Step 4: Determine the mass of CO₂ formed.

Note that the (maximum) mass of a product that can be formed is dictated by the limiting reagent. In this case, we will start at the number of moles of CO₂ formed from the limiting reagent (O₂) which is equal to 0.11022 mol.

The molar mass of CO₂ is 44.009 g.

Hence, 4.85 g of CO₂ can be formed.

------------------------------------------------------------

b. ANSWER:

The LR is O₂ and the ER is C₂H₄.

------------------------------------------------------------

c. SOLUTION:

The theoretical yield of the reaction is 4.85 g.

Hence, the percent yield of the reaction is 87.6%.

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Explanation:

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Answer:

Temperature is a measure of the average kinetic energy of the particles in a substance. Therefore, the substance with the least thermal energy would be the one with the lowest temperature and the lowest mass.

Using this information, we can see that the substance with the least thermal energy is 10 g of metal at 10°C. This is because it has both a lower temperature and a lower mass than the other substances listed. The other substances have a higher temperature and/or a higher mass, which means they have more kinetic energy and therefore more thermal energy.

The mass of chlorine in 4.75 mg of Freon-12 is approximately 1.39 x [tex]10^{-3}[/tex]g.

What is Mass?

Mass is a fundamental property of matter that measures the amount of substance or material present in an object. It is a scalar quantity and is typically measured in units such as grams (g) or kilograms (kg) in the metric system, or pounds (lb) or ounces (oz) in the imperial system.

Freon-12, also known as dichlorodifluoromethane, is a chlorofluorocarbon (CFC) compound that was used as a refrigerant and propellant in aerosol products. Its chemical formula is CCl2F2.

The atomic masses of carbon (C), chlorine (Cl), and fluorine (F) are approximately 12.01 g/mol, 35.45 g/mol, and 18.998 g/mol, respectively.

The molar mass of Freon-12 (CCl2F2) is:

Molar mass of Freon-12 = 12.01 g/mol (C) + 2 x 35.45 g/mol (Cl) + 2 x 18.998 g/mol (F)

= 120.91 g/mol

Next, we use the formula:

moles = mass / molar mass

to calculate the number of moles of Freon-12 in 4.75 mg:

moles of Freon-12 = 4.75 mg / 120.91 g/mol

= 3.92 x 10^-5 mol

Finally, we use Avogadro's number to calculate the number of molecules of Freon-12:

Number of molecules = moles of Freon-12 x Avogadro's number

= 3.92 x[tex]10^{-5}[/tex] mol x 6.022 x[tex]10^{23[/tex] molecules/mol

= 2.35 x [tex]10^{19}[/tex] molecules

To calculate the mass of chlorine in 4.75 mg of Freon-12, we can use the molar mass of chlorine (Cl) and the moles of Freon-12 calculated above.

The molar mass of chlorine (Cl) is 35.45 g/mol.

Mass of chlorine in Freon-12 = moles of Freon-12 x molar mass of chlorine

= 3.92 x [tex]10^{-5}[/tex] mol x 35.45 g/mol

= 1.39 x [tex]10^{-3}[/tex] g

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The  volume of acetone would be required to purify a 5.0g sample of compound is 58.82ml

Let use the solubility data of acetone provided to calculate the volume.

First we will need to calculate the solubility of Y in 25 degree.

   Solubility of Y= 0.12g/10ml= 0.012g/ml.

Solubility of y in boiling acetone = 0.85g/10ml =0.085g/ml.

In order to purify y, we need to dissolve the amount of y in the 5.0g sample.

The amount of acetone needed to dissolve y in the sample is

amount acetone= mass of y/ solubility of y in boiling acetone.

amount acetone= 5.0g/0.085g/ml= 58.82ml.

Therefore, the  volume of acetone would be required to purify a 5.0g sample of compound is 58.82ml

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1) Decomposition

2) Double replacement

3) Single replacement

4) Synthesis reaction

5) Single replacement

6) Synthesis reaction

7) Synthesis reaction

8) Single replacement

9) Double replacement

10) Synthesis reaction

11) Synthesis reaction

A chemical reaction is a process  that results in the conversion of one group of chemical compounds into another. In order to create a new material or substances, chemical bonds between atoms, ions, or molecules must be broken and formed. Reactants are the substances that start a chemical reaction, while products are the substances that come out of the process.

The law of conservation of mass requires that during a chemical process, the total amount of matter remains constant.

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Al₂(SO₄)₃ (ag) +2 K₃PO₄ (ag) → 2 AlPO₄ (s) + 3 K₂SO₄ (ag). This the balanced chemical equation. The sum of the coefficients of reaction is 7.

1) Name each component of the equation. Once the equation is balanced, the number of atoms of each kind must be equal on both sides.

2) What is each side of the equation's net charge? Once the equation is balanced, the net charge must be the same on both sides.

3) Start, if you can, with an element that is present in a single compound on each side of the equation. In order for the number of atoms of the element to be the same on both sides of the equation, adjust the coefficients (the numbers in front of the compound or molecule). To balance an equation, keep in mind that you must adjust the coefficients in the formulas, not the subscripts.

4) Once one element is balanced, proceed to balancing the other element. Continue until all components are in balance. It's simplest to finish with the elements present in their purest state.

5) Make sure the charge is balanced on both sides of the equation by checking your work.

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