Question

3O2(g) + 2CH3OH(l) → 2CO2(g) + 4H2O(l) Determine the amount of CO2(g) formed in the reaction if 4.20 moles of O2(g) reacts with an excess of CH3OH(l) and the percent yield of CO2(g) is 70.0%.

A. 1.86 moles

B. 3.57 moles

C. 4.00 moles

D. 1.96 moles

E. 2.16 moles

Answer 1

From balanced equation

Mol of CO2 formed = (2/3)*mol of O2 reacted

= (2/3)*4.20 mol

= 2.80 mol

Now use:

% yield = actual yield * 100 / theoretical yield

70.0 = actual yield * 100 / 2.80

actual yield = 1.96 mol

Answer: D