20 liters of hydrogen reacts with carbon to find the mass of the reaction product if the yield is from the theoretical possible 85%.
C + 2H2 = CH4
M (H2) = 2 g / mol.
M (CH4) = 16 g / mol.
Vm = 22.4 L / mol.
n (H2) = 20 / 22.4 = 0.89166 mol.
From the equation and stoichiometric coefficients, we see that the amount of hydrogen is twice the amount of methane.
n (CH4) = 0.89166 / 2 = 0.445 mol.
n = m / M => m = n * M,
m = 0.445 * 16 = 7.133 – theoretical yield (100%).
Then the practical yield ζ is 85% of 100%:
mpract = ζ * mtheor.
mpract = 0.85 * 7.133 = 6.03 g.
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