Answer to Question #259086 in General Chemistry for Alycia

Question

5.0 kg of hydrogen is reacted with 31 kg of oxygen. The experiment yields 28 kg of water. Calculate the percent yield of the reaction

Answer 1

2H₂ + O₂ → 2H₂O

M(H₂) = 2 g/mol

n(H₂) $= \frac{5000}{2} = 2500 \;mol$

M(O₂) = 32 g/mol

n(O₂) $= \frac{31000}{32} = 968.75 \;mol$

According to the reaction for one mole of O₂ we need two moles of H₂. So, O₂ is limiting reactant.

n(H₂O) = 2n(O₂) $= 2 \times 968.75 = 1937.5 \;mol$

M(H₂O) = 18 g/mol

m(H₂O)(theoretical) $= 1937.5 \times 18 = 34875 \;g = 34.875 \;kg$

Proportion:

37.875 kg – 100 %

28 kg – x

$x = \frac{28 \times 100}{37.875} = 73.927 \; \%$

Answer: 74 %