What's the matter, Jay. Does your teacher not like you any more. (Just kidding.) This was a slightly ugly problem. There are multiple steps, so stick with me. If there's something you don't follow, be sure to ask.
Givens:
mass of Cu2O + mass of CuO = 1.500 grams
mass of copper metal formed = 1.252 grams Cu
moles of copper metal formed = 0.0197 moles Cu
Define variables:
x moles Cu2O produces 2x moles Cu
y moles CuO produces y moles Cu
therefore 2x + y = 0.0197 mol Cu
and y = 0.0197 - 2x
Masses of each compound in mixture:
x moles Cu2O x 143.0g Cu2O / 1 mol Cu2O = 143x g Cu2O
y moles CuO x 79.5g CuO / 1 mol CuO = 79.5y g CuO
Total mass of mixture:
143x + 79.5y = 1.50 grams of the mixture
Substitute for y (recall y = 0.0197 - 2x):
143x + 79.5(0.0197 - 2x) = 1.50 g
Solve for moles:
143x +1.566 - 159x = 1.50 g
-16x = -0.066
x = 0.004125 moles Cu2O
y = 0.0197 - 2x = 0.01145 moles CuO
Convert moles to grams:
0.004125 mol Cu2O x 143.0 g Cu2O/1 mol Cu2O = 0.590 g Cu2O
0.01145 mole CuO x 79.5 g CuO/1 mol CuO = 0.910 g CuO
Now check the masses:
0.590 g Cu2O + 0.910 g CuO = 1.500 g of mixture
Compute percent composition:
0.590 g Cu2O / 1.500 g x 100 = 39.3% Cu2O
0.910 g CuO / 1.500 g x 100 = 60.7% CuO
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