20 liters of hydrogen reacts with carbon to find the mass of the reaction product if the yield is from

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.

Then:

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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