grade 11 chemistry scn3u test 5: stoichiometry
name:

| knowledge /13 | thinking/inquiry /15 | appl. /8 | comm. /10 |

true/false: indicate whether the statement is true or false. k/u-8
1. mole ratios that relate reactants to products can be constructed from the coefficients in a balanced chemical equation.
2. the amount of excess reactant dictates the amount of product formed in a chemical reaction.
3. in any chemical reaction, the theoretical yield will be less than or equal to the actual yield.
4. in a chemical reaction that involves two reactants, the limiting reagent is identified as the reactant that is entirely consumed.
5. the percentage yield is the actual amount of a product expressed as a percentage of the calculated theoretical yield of that product.
6. if 165.0 g of silver iodide was produced in a reaction for which the theoretical yield was 192.0 g, the percentage yield is 85.94%.
7. the following is an example of a balanced chemical equation:
2agno₃ + cacl₂ → 2agcl + ca(no₃)₂
8. a balanced chemical equation has the same number of each type of atom on each side of the equation.

completion k/u-5 complete each statement.
9. a (n) ______ reagent is the only reagent left over when all other reagents have been consumed in a chemical reaction.
10. a (n) ______ is a reagent that is completely consumed in a reaction and thereby limits the amount of product(s) that is/are formed.
11. when a balanced chemical equation is used to calculate the maximum amount of product that should form during a reaction, the value obtained is called the ______.
12. once a chemical reaction is actually carried out, the ratio of the actual yield to the theoretical yield is known as the ______.
13. ______ is the calculation of the quantities of reactants and products involved in a chemical reaction.

Question

grade 11 chemistry scn3u test 5: stoichiometry
name:

true/false: indicate whether the statement is true or false. k/u-8
1. mole ratios that relate reactants to products can be constructed from the coefficients in a balanced chemical equation.
2. the amount of excess reactant dictates the amount of product formed in a chemical reaction.
3. in any chemical reaction, the theoretical yield will be less than or equal to the actual yield.
4. in a chemical reaction that involves two reactants, the limiting reagent is identified as the reactant that is entirely consumed.
5. the percentage yield is the actual amount of a product expressed as a percentage of the calculated theoretical yield of that product.
6. if 165.0 g of silver iodide was produced in a reaction for which the theoretical yield was 192.0 g, the percentage yield is 85.94%.
7. the following is an example of a balanced chemical equation:
2agno₃ + cacl₂ → 2agcl + ca(no₃)₂
8. a balanced chemical equation has the same number of each type of atom on each side of the equation.

completion k/u-5 complete each statement.
9. a (n) ______ reagent is the only reagent left over when all other reagents have been consumed in a chemical reaction.
10. a (n) ______ is a reagent that is completely consumed in a reaction and thereby limits the amount of product(s) that is/are formed.
11. when a balanced chemical equation is used to calculate the maximum amount of product that should form during a reaction, the value obtained is called the ______.
12. once a chemical reaction is actually carried out, the ratio of the actual yield to the theoretical yield is known as the ______.
13. ______ is the calculation of the quantities of reactants and products involved in a chemical reaction.

Accepted Answer

### True/False Questions:
1. **Explanation**: Mole ratios are determined by the coefficients in a balanced chemical equation, relating reactants and products.
   **Answer**: True (T)

2. **Explanation**: The limiting reactant (not excess) determines the amount of product formed.
   **Answer**: False (F)

3. **Explanation**: Theoretical yield is the maximum possible; actual yield is often less (due to inefficiencies), so theoretical yield ≥ actual yield.
   **Answer**: False (F)

4. **Explanation**: The limiting reagent is fully consumed, limiting product formation.
   **Answer**: True (T)

5. **Explanation**: Percentage yield = (Actual Yield / Theoretical Yield) × 100, so it’s actual as a percentage of theoretical.
   **Answer**: True (T)

6. **Explanation**: Calculate percentage yield: $ \frac{165.0\ \text{g}}{192.0\ \text{g}} \times 100 = 85.9375\% \approx 85.94\% $.
   **Answer**: True (T)

7. **Explanation**: Count atoms: Left: 2 Ag, 2 N, 6 O, 1 Ca, 2 Cl; Right: 2 Ag, 2 N, 6 O, 1 Ca, 2 Cl. Balanced.
   **Answer**: True (T)

8. **Explanation**: A balanced equation has equal numbers of each atom on both sides.
   **Answer**: True (T)

### Completion Questions:
9. **Explanation**: The reagent left over after others are consumed is the excess reagent.
   **Answer**: excess

10. **Explanation**: The reagent fully consumed, limiting product, is the limiting reagent.
    **Answer**: limiting reagent

11. **Explanation**: The maximum product calculated from a balanced equation is the theoretical yield.
    **Answer**: theoretical yield

12. **Explanation**: (Actual Yield / Theoretical Yield) × 100 is percentage yield, but the ratio (without ×100) is sometimes called yield efficiency, but here it’s percentage yield (or just yield, but contextually percentage yield). Wait, no: The ratio (Actual/ Theoretical) × 100 is percentage yield. But the question says “ratio of actual to theoretical yield” (not ×100). Wait, no—recheck: “the ratio of the actual yield to the theoretical yield” is the **percentage yield** (when multiplied by 100), but the term for the ratio (Actual/Theoretical) is sometimes “yield fraction,” but in stoichiometry, the term is **percentage yield** (since it’s expressed as a percentage). Wait, no: The question says “the ratio of the actual yield to the theoretical yield is known as the ______.” Actually, the percentage yield is (Actual/Theoretical) × 100, so the ratio (Actual/Theoretical) is the “yield ratio,” but in standard terms, the term is **percentage yield** (even though it’s a percentage, the ratio is the basis). Wait, no—let’s check definitions: Percentage yield = (Actual Yield / Theoretical Yield) × 100. So the ratio (Actual/Theoretical) is the “yield fraction,” but the term here is **percentage yield** (since it’s the ratio expressed as a percentage). Wait, maybe the question expects “percentage yield,” but let’s confirm. Alternatively, “yield” but no—standard term is **percentage yield**.

Wait, no—re-reading: “the ratio of the actual yield to the theoretical yield” (not multiplied by 100) is sometimes called the “yield efficiency,” but in stoichiometry, the term is **percentage yield** (because it’s typically expressed as a percentage). So the answer is **percentage yield**? Wait, no—let’s check a textbook: “The percentage yield is the ratio of the actual yield to the theoretical yield, multiplied by 100.” So the ratio (Actual/Theoretical) is the “yield fraction,” but the term for the ratio (when multiplied by 100) is percentage yield. But the question says “the ratio of the actual yield to the theoretical yield is known as the ______.” So maybe the answer is **percentage yield** (even though it’s a percentage, the ratio is the basis). Alternatively, maybe “yield,” but no. Let’s go with **percentage yield**.

13. **Explanation**: The calculation of reactant and product quantities in a reaction is stoichiometry.
    **Answer**: Stoichiometry

### Final Answers (True/False):
1. T
2. F
3. F
4. T
5. T
6. T
7. T
8. T

### Final Answers (Completion):
9. excess
10. limiting reagent
11. theoretical yield
12. percentage yield
13. Stoichiometry

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