Use the chemical reaction below to answer
the questions that follow.
CuO(s) + H2(g) → Cu(s) + H2O(g)
a. What is the limiting reactant when 19.9 g
CuO react with 2.02 g H2?
b. The actual yield of copper was 15.0 g.
What is the percentage yield?
c. How many grams of Cu can be collected
if 20.6 g CuO react with an excess of
hydrogen with a yield of 91.0%?
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To answer these questions, we need to use the concept of the limiting reactant and percent yield in chemical reactions.
a. To determine the limiting reactant, we compare the amount of CuO and H2 and calculate the number of moles for each.
1. Convert the mass of CuO to moles:
Molar mass of CuO = atomic mass of Cu + atomic mass of O = 63.55 g/mol + 16.00 g/mol = 79.55 g/mol
Number of moles of CuO = mass / molar mass = 19.9 g / 79.55 g/mol = 0.25 mol
2. Convert the mass of H2 to moles:
Molar mass of H2 = 2 g/mol
Number of moles of H2 = mass / molar mass = 2.02 g / 2 g/mol = 1.01 mol
3. Compare the moles of CuO and H2:
The stoichiometric ratio between CuO and H2 is 1:1. From the balanced equation, we can see that 1 mole of CuO reacts with 1 mole of H2. Therefore, CuO and H2 are in a 1:1 ratio.
Since the moles of CuO (0.25 mol) are less than the moles of H2 (1.01 mol), CuO is the limiting reactant.
b. To calculate the percentage yield, we need the actual yield and the theoretical yield.
1. Theoretical yield:
From the balanced equation, we can see that 1 mole of CuO produces 1 mole of Cu. Therefore, the theoretical yield of Cu can be calculated from the moles of CuO used.
Moles of CuO = 20.6 g / 79.55 g/mol = 0.26 mol
Theoretical yield of Cu = 0.26 mol
2. Percentage yield:
Percentage yield = (actual yield / theoretical yield) x 100
Percentage yield = (15.0 g / 0.26 mol) x 100 = 5769%
c. To calculate the mass of Cu collected, we need the moles of CuO used and the yield percentage.
1. Convert the moles of CuO to mass:
Moles of CuO = 20.6 g / 79.55 g/mol = 0.26 mol
2. Calculate the yield of Cu:
Yield of Cu = moles of CuO used x yield percentage
Yield of Cu = 0.26 mol x 0.91 = 0.2366 mol
3. Convert the moles of Cu to mass:
Molar mass of Cu = 63.55 g/mol
Mass of Cu = moles of Cu x molar mass of Cu
Mass of Cu = 0.2366 mol x 63.55 g/mol = 15.03 g
Therefore, the mass of Cu that can be collected is 15.03 g.