C7H6O3+CH3OH→C8H8O3+H2O

Question

In any experiment, 1.50g of salicyclic acid is reacted with 11.20g of methanol. The yield of methyl salicylate, C8H8O3, is 1.31g. What is the percent yield?

From my understanding the equation is already balanced, correct?

My answer: 26.7%, is this correct?

Work: (11.20gCH3OH)(1 mol CH3OH)/32.05gCH3OH=0.3495gCH3OH

0.3495g/1.31g= 26.68%

Answer 1

You know it is a limiting reagent problem when BOTH reactants are given.
1. Write the equation and balance it. I think everything is 1:1:1:1

2a. Convert 11.2 grams methanol to moles. moles = grams/molar mass.
2b. Convert 1.5 g salicylic acid to moles the same way.

3a. Using the coefficients in the balanced equation, convert moles methanol to moles of methyl salicylate.
3b. Using same procedure, convert moles salicylic acid to moles methyl salicylate.
3c. It is more than likely that the answers to 3a and 3b will be different which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reactant providing that smaller value is the limiting reagent.
4. Convert the value from 3c to grams. g = moles x molar mass. This is the theoretical yield.
5. Percent yield = (actual yield/theoretical yield)*100 = ??

Answer 2

I am still getting the same answer

Answer 3

76.9