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Reactions do not always go the way a problem predicts that they will. Textbook problems provide theoretical, or "perfect" solutions. Laboratory experiences provide actual, or "real" solutions. Actual
solutions are never the same as the theoretical solutions, because there is always a source of error. To determine the efficiency of a reaction, chemists calculate its percent yield. Percent yield is defined as:
(Actual Value/Theoretical Value) X 100.
Theoretical values can be calculated, but actual values are provided within the problem. This quiz will cover simple percent yield problems. You will need a calculator and a periodic table. Select the best answer from the given choices.
Al(OH)3 + 3HCl --> What are the products of this reaction?
AlH3 and HCl
AlCl3 and H2O
AlCl3 and OH3
AlCl and OH3
Al(OH)3 + 3HCl --> 3H2O + AlCl3 If you have 14.0 grams of aluminum hydroxide, how much aluminum chloride is produced?
23.9g
34.5g
30g
12.56g
Al(OH)3 + 3HCl --> 3H2O + AlCl3 If you actually recovered 22.0 grams of aluminum chloride, what is the percent yield of the reaction?
76%
88%
92%
100%
Al(OH)3 + 3HCl --> 3H2O + AlCl3 f you have 14.0 grams of aluminum hydroxide, how much water is produced?
8g
9.68g
9g
6.78g
Al(OH)3 + 3HCl --> 3H2O + AlCl3 If you recovered 8.5g of water from the reaction, what is the percent yield?
88%
98%
100%
78%
In one container, 10.00 kg of salicylic acid is mixed with 10.00 kg of acetic anhydride. Which reactant is limiting? Which is in excess?
Aspirin is the limiting reagent.
Salicylic acid is the limiting reagent.
Acetic anhydride is the limiting reagent.
None of these
In a chemistry experiment, a student obtained 5.68 g of a product. What is the percent yield of the product if the theoretical yield was 7.12 g?
67%
79.8%
80%
87%
What is the theoretical yield of Ca(OH)2, in grams, if 39.27 g of CaO is hydrolyzed (reacted) in an excess of water?
55 g
50 g
51.9 g
41.9 g
