Percentage Yield (chemistry Only) (GCSE Chemistry)

Which calculation gives percentage yield when given moles: theoretical moles = 0.250 mol and actual moles = 0.190 mol?

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

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

Which laboratory technique helps improve percentage yield by preventing product loss during transfer?

A student reports percentage yield to two significant figures as 87%. Which of these actual calculations is consistent? (theoretical 14.5 g)

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?

You obtain 2.40 g product but after drying it still contains 0.10 g solvent. The theoretical mass is 2.50 g. Which is the correct percentage yield (use dry mass)?

A student obtains very different yields in four repeats (random scatter). Which best practice reduces random error and gives a better percentage yield estimate?

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

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

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.