A 1.60 g sample of containing potassium hydrogen carbonate is decomposed with heat into potassium carbonate and carbonic acid. what is the actual yield of potassium carbonate if this reaction proceeded with 92% efficiency?

##1.0156## grams ##K_2CO_3##

1. Take the balanced equation; ##2KHCO_3->K_2CO_3+H_2CO_3##
2. Take the molar masses of ##KHCO_3## and ##K_2CO_3##
3. Compute stoichiometrically, starting with the mass of ##KHCO_3## ##1.6cancel(g KHCO_3) ##x## (1 cancel(mol KHCO_30)/(cancel(100g KHCO_3)) ##x## (1 cancel(mol K_2CO_3))/(2 cancel(mol KHCO_3)) ##x## (138g K_2CO_3)/(1 cancel(mol K_2CO_3))##
4. The answer is ##1.104## g ##K_2CO_3##
5. To compute the atual yield, use the formula: ##% yield=(actual yield)/(theo yield)##, rearrange and plug in values to the derived formula; ##actual yied=(% yield)(theo yield)##
6. The actual yield is ##1.0156g## ##K_2CO_3##