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 carried out a titration to produce a precipitate, filtered it and weighed wet filter plus precipitate, then calculated yield. This gave a percentage yield of 110%. Best immediate correction?

Which action would increase percentage yield of a crystallised salt product?

A chemist reports a percentage yield of 0% for a reaction. Which is the most likely interpretation?

A chemist expects theoretical mass 5.00 g. He obtains 4.20 g on first run, repeats protocol identically and obtains 4.25 g. Which value should be used as actual yield when reporting % yield?

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

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

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.)?

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)?

If the theoretical mole yield of product is 0.500 mol and the actual mole yield is 0.420 mol, what is the percentage yield?

When calculating percentage yield using masses, why must you convert masses to moles if reaction equation involves mole ratios?