Percentage Yield (chemistry Only) (GCSE Chemistry)

Theoretical yield = 0.375 mol, molar mass product = 88.0 g/mol, actual mass obtained = 27.5 g. What is percentage yield?

A student makes a salt and gets a measured mass higher than expected. Which lab error would cause an erroneously low calculated percentage yield (i.e., you think yield smaller than it really is)?

Hydrogen + chlorine ? hydrogen chloride. Theoretical yield of HCl = 36.5 g; actual yield = 29.2 g. What is percentage yield (to 3 s.f.)?

Which of these reasons explains a low percentage yield (e.g., 45%)?

A student’s measured actual yield is higher than the theoretical yield calculated using balanced equation and pure reactants. Best explanation?

Calcium carbonate is heated to give calcium oxide. Theoretical mass of CaO = 12.0 g but student obtains 10.0 g. What is the percentage yield (to 3 s.f.)?

If the maximum theoretical mass of a salt is 25.0 g and a student obtains 20.0 g, what is the percentage yield?

Theoretical yield of a product is 12.4 g and the actual mass obtained is 9.3 g. What is the percentage yield (to the nearest whole %)?

If theoretical yield is based on limiting reagent but the student used excess of the other reagent, what happens to theoretical yield?

A student calculates percentage yield using the formula: percentage yield = (mass of product actually obtained / maximum theoretical mass of product) × 100.

A reaction produces theoretical gaseous product volume 24.0 dm3 but measured collection is 19.2 dm3. What is percentage yield?