Percentage Yield (chemistry Only) (GCSE Chemistry)

When calculating theoretical yield you must base the calculation on the limiting reagent. Which statement is correct?

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.)?

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

A student expects 5.00 g of a product (theoretical) but recovers only 4.50 g. Which experimental factor would directly reduce percentage yield?

A reaction gives a percentage yield greater than 100%. Which is the most likely reason?

The maximum theoretical mass of a salt is 12.5 g and the percentage yield is 92.8%. Calculate the actual mass of salt produced.

Which statement about reporting percentage yield is correct?

A theoretical yield requires calculations using balanced equation. For 2A + 3B ? 4C, if you start with 0.500 mol A and excess B, how many moles of C are theoretically possible?

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

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