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- 1. Multiple ChoiceThe ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect settingPercentactualstoichiometrytheoretical
- 2. Multiple Choice
When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?
90.4%
104%
96.15%
1.04%
- 3. Multiple ChoiceTheoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.1.16%116%85%76% - 4. Multiple ChoiceIn a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?82%0.82%10.1 %100%
- 5. Multiple ChoiceBalance the following reaction :
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)1,2,2,21,2,1,12,1,1,12,1,2,1 - 6. Multiple ChoiceUsing the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?4 moles Fe6 moles Fe9 moles Fe2 moles Fe - 7. Multiple Choice2H2 + O2 → 2H2O
How many moles of water can be produced if 8 moles H2 are used?4 moles8 moles16 moles2 moles - 8. Multiple ChoiceTheoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.1.16%116%85%76% - 9. Multiple Choice
Reactant and products might adhere to containers causing actual yield to be less than theoretical yield.
true
false
- 10. Multiple Choice
Competing reactions might occur forming other products causing your actual yield to be less than your theoretical yield.
true
false
- 11. Multiple Choice
Some product can be transformed completely into energy causing your actual yield to be less than your theoretical yield.
true
false
- 12. Multiple Choice
Some product may be lost during filtering causing your actual yield to be less than your theoretical yield.
true
false
- 13. Multiple ChoiceN2 + 3H2 → 2NH3
How many moles of hydrogen are needed to react with 2 moles of nitrogen?6231 - 14. Multiple Choice
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%actual yield; theoretical yieldtheoretical yield; actual yield - 15. Multiple ChoiceWhat is the molar mass of Carbon?6122040
- 16. Multiple ChoiceHow many moles is 4 grams of Calcium?0.10 moles10 moles44 moles160 moles
- 17. Multiple ChoiceWhat is Avogadro's Number?602,00023 x 10610 x 10236.02 x 1023
- 18. Multiple Choice
In the image, which reactant is limiting?
The white molecules, because there are extra.
The black atoms, because they are completely used up.
The white molecules, because they are completely used up.
The black atoms, because there are extra.
- 19. Multiple ChoiceIf a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating thetheoretical yieldmole ratioactual yieldpercentage yield
- 20. Multiple Choice7. The amount of product that actually forms when a chemical reaction is carried out in a laboratory is called the _________ yield.actualtheoreticalpercent
- Answer choicesTagsAnswer choicesTags