Stoichiometry Trivia Test: MCQ Quiz!

In order to determine the limiting reactant, we need to compare the amount of ammonia and copper (II) oxide used in the reaction. The molar mass of ammonia (NH3) is 17.03 g/mol, so 40g of ammonia is approximately 2.35 moles. The molar mass of copper (II) oxide (CuO) is 79.55 g/mol, so 80.0g of copper (II) oxide is approximately 1.00 mole. Since the molar ratio between ammonia and copper (II) oxide is 2:1, we can see that there are more moles of ammonia than copper (II) oxide. Therefore, copper (II) oxide is the limiting reactant in this reaction.

When copper(II) oxide is heated with hydrogen gas, a chemical reaction occurs and water and copper metal are produced. The balanced chemical equation for this reaction is: CuO + H2 → Cu + H2O. According to the equation, 1 mole of copper(II) oxide (CuO) reacts to produce 1 mole of copper (Cu). To find the mass of copper that can be obtained, we need to convert the mass of copper(II) oxide (32.0g) to moles using its molar mass (79.55g/mol), and then use the mole ratio from the balanced equation to find the mass of copper produced. The calculation gives us a mass of approximately 25.5g of copper.

The coefficients that balance the equation are 2, 1, 2. This means that 2 molecules of nitrogen monoxide react with 1 molecule of oxygen gas to produce 2 molecules of nitrogen dioxide. The balanced equation is 2NO + O2 -> 2NO2.

The balanced chemical equation for the reaction between ammonia, copper (II) oxide, and copper is 2NH3 + 3CuO -> 3Cu + 3H2O + N2. This equation shows that 2 moles of ammonia react with 3 moles of copper (II) oxide to produce 3 moles of copper, 3 moles of water, and 1 mole of nitrogen gas. Therefore, the coefficients for the balanced chemical equation are 2, 3, 3, 3, 1.

The mass of nitrogen gas produced in the reaction is 9.4 g.

The theoretical yield of hydrogen gas can be calculated using the stoichiometry of the reaction. The balanced equation for the decomposition of water is 2H2O -> 2H2 + O2. From the equation, we can see that for every 2 moles of water, we get 2 moles of hydrogen gas. The molar mass of water is 18.02 g/mol, so 36.0 g of water is equal to 2 moles. Therefore, the theoretical yield of hydrogen gas is also 2 moles, which is equal to 4.04 g H2.

Ammonia is the excess reactant, meaning it will not be completely used up in the reaction. To determine how much is left over, a mass-mass problem can be used. The given mass of copper(II) oxide (CuO) is 80g, and the mass of ammonia is the unknown. The answer, 28.6g, represents the amount of ammonia that is used up in the reaction, while the remaining amount is the excess reactant that remains.