Question

A strip of copper (II) with a mass of 1.05 g is placed in a beaker that contains excess silver nitrate solution. When the silver crystals were washed, dried, and massed, the percentage yield was found to be 92.4%. What was the actual/experimental yield of silver produced?

a) 1.07 g
b) 1.14 g
c) 1.27 g
d) 1.37 g

Answer 1

The actual/experimental yield of silver produced can be calculated using the percentage yield. The percentage yield is the actual yield divided by the theoretical yield, multiplied by 100. In this case, the percentage yield is given as 92.4%. The theoretical yield can be calculated by multiplying the mass of copper (II) with the molar ratio between copper (II) and silver. The mass of copper (II) is given as 1.05 g and the molar ratio is 1:1, so the theoretical yield of silver is 1.05 g. To find the actual yield, we can use the percentage yield formula: Actual Yield = Percentage Yield x Theoretical Yield. Therefore, the actual/experimental yield of silver produced is approximately 0.9687 g.

Step-by-step explanation:

The actual/experimental yield of silver produced can be calculated using the percentage yield. The percentage yield is the actual yield divided by the theoretical yield, multiplied by 100. In this case, the percentage yield is given as 92.4%. The theoretical yield can be calculated by multiplying the mass of copper (II) with the molar ratio between copper (II) and silver. The mass of copper (II) is given as 1.05 g and the molar ratio is 1:1, so the theoretical yield of silver is 1.05 g. To find the actual yield, we can use the percentage yield formula:

Actual Yield = Percentage Yield x Theoretical Yield

Actual Yield = 0.924 x 1.05 g = 0.9687 g

Therefore, the actual/experimental yield of silver produced is approximately 0.9687 g.

Answer 2

This choice corresponds to the actual yield calculated from the given experimental yield and mass of copper (II), utilizing the percentage yield formula.The experimental yield of silver produced is 1.14 g.Therefore the correct answer is b) 1.14 g.

Step-by-step explanation:

In a chemical reaction involving copper (II) and silver nitrate, a strip of copper (II) with a mass of 1.05 g was used. The reaction resulted in the formation of silver crystals. After washing, drying, and measuring, the experimental yield was found to be 92.4%.

To determine the actual yield, we use the formula for percentage yield:

`\[ \text{Percentage Yield} = \left( \frac{\text{Experimental Yield}}{\text{Actual Yield}} \right) * 100 \]`

Rearranging the formula to solve for the actual yield:

`\[ \text{Actual Yield} = \left( \frac{\text{Experimental Yield}}{\text{Percentage Yield}} \right) * 100 \]`

Substituting the given values:

`\[ \text{Actual Yield} = \left( \frac{1.05 \, \text{g}}{92.4} \right) * 100 \]`

Calculating this gives us the actual yield of silver, which is approximately 1.14 g. Therefore, the answer is Option b.

It's crucial to understand that the percentage yield represents the efficiency of the reaction, indicating how much of the theoretically predicted product was obtained in reality.

In this case, achieving a 92.4% yield implies a successful and relatively efficient conversion of copper (II) to silver. The slight deviation from 100% could be attributed to factors like incomplete reactions or losses during the experimental process.