Chemistry College

1.) How many grams of aluminum hydroxide can be produced from the
synthesis reaction of 24.3 g of aluminum oxide and 82.1 g of water?

Answers

Answer 1

Answer: 37.1 grams of aluminum hydroxide can be produced from the given amounts of aluminum oxide and water

Explanation:

The balanced chemical equation for the synthesis of aluminum hydroxide from aluminum oxide and water is:

Al2O3 + 3H2O -> 2Al(OH)3

From the equation, we can see that 1 mole of Al2O3 reacts with 3 moles of H2O to produce 2 moles of Al(OH)3.

We need to first calculate the number of moles of Al2O3 and H2O we have:

Number of moles of Al2O3 = mass / molar mass = 24.3 g / 101.96 g/mol = 0.238 moles

Number of moles of H2O = mass / molar mass = 82.1 g / 18.02 g/mol = 4.56 moles

From the balanced equation, we know that 1 mole of Al2O3 produces 2 moles of Al(OH)3. So, the number of moles of Al(OH)3 produced will be:

Number of moles of Al(OH)3 = (0.238 mol Al2O3) x (2 mol Al(OH)3 / 1 mol Al2O3) = 0.476 mol Al(OH)3

Finally, we can calculate the mass of Al(OH)3 produced:

Mass of Al(OH)3 = number of moles x molar mass = 0.476 mol x 78.0 g/mol = 37.1 g

Therefore, 37.1 grams of aluminum hydroxide can be produced from the given amounts of aluminum oxide and water.

Related Questions

Beer's Law becomes nonlinear at high analyte concentrations
true or false

Answers

Answer:

True

Explanation:

Self-absorption occurs when the absorbing species in a sample interacts with other absorbing species in the same sample, leading to an overestimation of the absorbance and a deviation from the linear relationship described by Beer's Law. Therefore, at high analyte concentrations, the linear relationship breaks down and the law becomes nonlinear...

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