Answer to Question #181069 in General Chemistry for lala

Question

A hundred grams of Sulfuric acid yielded ten grams of water.

H2SO4(l) = H2O(l) + SO3(l)

a. Balance the chemical equation;

b. Identify the limiting reactant and the excess reactant if applicable;

c. Compute for the theoretical yield; d. Determine the percent yield of the reaction;

e. Calculate the percent error and

f. Compute for the excess amount of the excess reactant if applicable.

g. Show the complete solutions for your answers in a separate paper.

Answer 1

Balanced

H2SO4(l) = H2O(l) + SO3(l)

Moles of H2SO4 = $\frac{100}{98}=1.02 moles$

Moles of H2O $=1.02 moles$

Not applicable for limiting and excess reactant

Theoretical yield = 1.02 × 18=18.36 g

Percent yield = $\frac{18}{18.36}×100=98$ %