Use The Balanced Equation 2 H 2 SO 4 + Cu → SO 2 + 2 H 2 O + CuSO 4 2 \text{H}_2\text{SO}_4 + \text{Cu} \rightarrow \text{SO}_2 + 2 \text{H}_2\text{O} + \text{CuSO}_4 2 H 2 ​ SO 4 ​ + Cu → SO 2 ​ + 2 H 2 ​ O + CuSO 4 ​ To Answer The Following Question.A Chemist Is Trying To Find The Percent Yield Of The Reaction Above. If He Reacts

Understanding Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction. It is defined as the ratio of the actual yield of a product to its theoretical yield, multiplied by 100. In other words, it is a measure of how much of the product is actually obtained compared to the amount that is expected to be obtained based on the balanced equation of the reaction.

The Balanced Equation

The balanced equation for the reaction between sulfuric acid (H2SO4) and copper (Cu) is:

$$2 \text{H}_2\text{SO}_4 + \text{Cu} \rightarrow \text{SO}_2 + 2 \text{H}_2\text{O} + \text{CuSO}_4$$

Theoretical Yield

To calculate the percent yield, we first need to calculate the theoretical yield of the product (CuSO4). The theoretical yield is the amount of product that is expected to be obtained based on the balanced equation of the reaction.

The molar mass of CuSO4 is 159.62 g/mol. The molar mass of Cu is 63.55 g/mol. The molar mass of SO4 is 96.06 g/mol.

Let's assume that 100 g of Cu is reacted with 200 g of H2SO4. We can calculate the number of moles of Cu that is reacted as follows:

$$\text{moles of Cu} = \frac{\text{mass of Cu}}{\text{molar mass of Cu}} = \frac{100 \text{ g}}{63.55 \text{ g/mol}} = 1.573 \text{ mol}$$

Since the balanced equation shows that 1 mole of Cu reacts with 2 moles of H2SO4, we can calculate the number of moles of H2SO4 that is reacted as follows:

$$\text{moles of H}_2\text{SO}_4 = 2 \times \text{moles of Cu} = 2 \times 1.573 \text{ mol} = 3.146 \text{ mol}$$

The number of moles of CuSO4 that is produced is equal to the number of moles of Cu that is reacted, which is 1.573 mol.

The mass of CuSO4 that is produced can be calculated as follows:

$$\text{mass of CuSO}_4 = \text{moles of CuSO}_4 \times \text{molar mass of CuSO}_4 = 1.573 \text{ mol} \times 159.62 \text{ g/mol} = 251.9 \text{ g}$$

Therefore, the theoretical yield of CuSO4 is 251.9 g.

Actual Yield

The actual yield of CuSO4 is the amount of product that is actually obtained. Let's assume that the actual yield of CuSO4 is 220 g.

Calculating Percent Yield

The percent yield can be calculated as follows:

$$\text{percent yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100$$

Substituting the values, we get:

$$\text{percent yield} = \frac{220 \text{ g}}{251.9 \text{ g}} \times 100 = 87.4\%$$

Therefore, the percent yield of the reaction is 87.4%.

Conclusion

In conclusion, percent yield is a measure of the efficiency of a chemical reaction. It is defined as the ratio of the actual yield of a product to its theoretical yield, multiplied by 100. The balanced equation for the reaction between sulfuric acid (H2SO4) and copper (Cu) is:

$$2 \text{H}_2\text{SO}_4 + \text{Cu} \rightarrow \text{SO}_2 + 2 \text{H}_2\text{O} + \text{CuSO}_4$$

The theoretical yield of CuSO4 is 251.9 g, and the actual yield is 220 g. The percent yield of the reaction is 87.4%.

Importance of Percent Yield

Percent yield is an important concept in chemistry because it helps us to understand the efficiency of a chemical reaction. It is a measure of how much of the product is actually obtained compared to the amount that is expected to be obtained based on the balanced equation of the reaction.

Factors Affecting Percent Yield

There are several factors that can affect the percent yield of a reaction. These include:

• Impurities: Impurities in the reactants can affect the percent yield of the reaction.
• Incomplete reaction: If the reaction is not complete, the percent yield will be lower than expected.
• Loss of product: If the product is lost during the reaction or after the reaction, the percent yield will be lower than expected.
• Instrumental errors: Instrumental errors can also affect the percent yield of the reaction.

Conclusion

In conclusion, percent yield is an important concept in chemistry that helps us to understand the efficiency of a chemical reaction. It is a measure of how much of the product is actually obtained compared to the amount that is expected to be obtained based on the balanced equation of the reaction. The balanced equation for the reaction between sulfuric acid (H2SO4) and copper (Cu) is:

$$2 \text{H}_2\text{SO}_4 + \text{Cu} \rightarrow \text{SO}_2 + 2 \text{H}_2\text{O} + \text{CuSO}_4$$

Q: What is percent yield?

A: Percent yield is a measure of the efficiency of a chemical reaction. It is defined as the ratio of the actual yield of a product to its theoretical yield, multiplied by 100.

Q: Why is percent yield important?

A: Percent yield is an important concept in chemistry because it helps us to understand the efficiency of a chemical reaction. It is a measure of how much of the product is actually obtained compared to the amount that is expected to be obtained based on the balanced equation of the reaction.

Q: How do I calculate percent yield?

A: To calculate percent yield, you need to know the actual yield of the product and the theoretical yield of the product. The theoretical yield is the amount of product that is expected to be obtained based on the balanced equation of the reaction. The actual yield is the amount of product that is actually obtained.

The formula for calculating percent yield is:

$$\text{percent yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100$$

Q: What are some common mistakes to avoid when calculating percent yield?

A: Some common mistakes to avoid when calculating percent yield include:

• Not using the correct units: Make sure to use the correct units for the actual yield and the theoretical yield.
• Not rounding correctly: Make sure to round the actual yield and the theoretical yield to the correct number of significant figures.
• Not considering instrumental errors: Instrumental errors can affect the percent yield of the reaction, so make sure to consider them when calculating the percent yield.

Q: How do I determine the theoretical yield of a product?

A: To determine the theoretical yield of a product, you need to know the balanced equation of the reaction and the molar masses of the reactants and products. The theoretical yield is the amount of product that is expected to be obtained based on the balanced equation of the reaction.

The formula for calculating the theoretical yield of a product is:

$$\text{theoretical yield} = \text{moles of reactant} \times \text{molar mass of product}$$

Q: What are some common factors that can affect the percent yield of a reaction?

A: Some common factors that can affect the percent yield of a reaction include:

• Impurities: Impurities in the reactants can affect the percent yield of the reaction.
• Incomplete reaction: If the reaction is not complete, the percent yield will be lower than expected.
• Loss of product: If the product is lost during the reaction or after the reaction, the percent yield will be lower than expected.
• Instrumental errors: Instrumental errors can also affect the percent yield of the reaction.

Q: How do I report the percent yield of a reaction?

A: When reporting the percent yield of a reaction, make sure to include the following information:

• The actual yield of the product: Report the actual yield of the product in the correct units.
• The theoretical yield of the product: Report the theoretical yield of the product in the correct units.
• The percent yield: Report the percent yield as a percentage.

For example:

"The actual yield of the product was 220 g, the theoretical yield was 251.9 g, and the percent yield was 87.4%."

Conclusion

In conclusion, percent yield is an important concept in chemistry that helps us to understand the efficiency of a chemical reaction. It is a measure of how much of the product is actually obtained compared to the amount that is expected to be obtained based on the balanced equation of the reaction. By following the steps outlined in this article, you can calculate the percent yield of a reaction and report it accurately.