The theoretical yield of a reaction is the amount of product obtained if the lim

Question

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: CO (g) + 2 H_2 (g) rightarrow CH_3OH (l) If 13.83 g of CO are mixed with 7.02 g H_2. what is the theoretical yield (in grams) of CH_3OH produced by the reaction? Calculate the amount of each reactant, in moles, initially present using the molar mass of each reactant Calculate the quantity, in moles, of product complete consumption of the limiting reactant Compare the ratio of moles of reactants present to the ratio of the stoichiometric coefficients of the reactants to determine which is the limiting reactant. Calculate the mass of product formed based molar mass of the product.

Explanation / Answer

we know that

moles = mass / molar mass

so

moles of CO = 13.83 / 28 = 0.494

moles of H2 = 7.02 / 2 = 3.51

now

the reaction is

CO + 2 H2 --> CH3OH

we can see that

moles of H2 required = 2 x moles of CO

moles of H2 required = 2 x 0.494 = 0.988

but 3.51 moles of H2 are present

so

H2 is in excess and CO is the limiting reagent

CO + 2H2 --> CH3OH

we can see that

theoreitcal moles of CH3OH produced = moles of CO taken

theoretical moles of CH3OH produced = 0.494

now

mass = moles x molar mass

molar mass of CH3OH = 32 g/mol

so

theoretical mass fo CH3OH = 0.494 x 32 = 15.8

so

15.8 grams is the theoretical yield of CH3OH

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