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[tex] \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + H_2O [/tex]

1. If 30 g of HCl is reacted with excess NaOH, and 10 g of NaCl is produced, what is the theoretical yield of the experiment?

2. If 30 g of HCl is reacted with excess NaOH, and 10 g of NaCl is produced, what is the percent yield of the experiment?

Sagot :

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To answer the given question, we need to perform calculations in two parts: finding the theoretical yield of NaCl and determining the percent yield of the experiment.

### Part 1: Theoretical Yield

1. Calculate the number of moles of HCl:

- The molar mass of HCl (hydrochloric acid) is calculated using the atomic masses of hydrogen (H) and chlorine (Cl):
[tex]\[ \text{Molar mass of } \text{HCl} = 1 \text{ (H)} + 35.5 \text{ (Cl)} = 36.5 \text{ g/mol} \][/tex]

- Given mass of HCl is 30 grams. The number of moles of HCl can be found using the formula:
[tex]\[ \text{Moles of HCl} = \frac{\text{Mass of HCl}}{\text{Molar mass of HCl}} = \frac{30 \text{ g}}{36.5 \text{ g/mol}} \approx 0.8219 \text{ moles} \][/tex]

2. Determine the moles of NaCl produced:

According to the balanced chemical equation, 1 mole of HCl produces 1 mole of NaCl. Hence, the moles of NaCl will be the same as the moles of HCl:
[tex]\[ \text{Moles of NaCl} = 0.8219 \][/tex]

3. Calculate the theoretical yield of NaCl:

- The molar mass of NaCl (sodium chloride) is calculated using the atomic masses of sodium (Na) and chlorine (Cl):
[tex]\[ \text{Molar mass of NaCl} = 23 \text{ (Na)} + 35.5 \text{ (Cl)} = 58.5 \text{ g/mol} \][/tex]

- The theoretical yield (mass) of NaCl can be found using the moles of NaCl and its molar mass:
[tex]\[ \text{Theoretical yield of NaCl} = \text{Moles of NaCl} \times \text{Molar mass of NaCl} = 0.8219 \text{ moles} \times 58.5 \text{ g/mol} \approx 48.08 \text{ grams} \][/tex]

### Part 2: Percent Yield

Percent yield is calculated by comparing the actual yield to the theoretical yield using the formula:
[tex]\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \][/tex]

Given:
- Actual yield (observed mass of NaCl) = 10 grams
- Theoretical yield of NaCl = 48.08 grams

Substitute these values into the percent yield formula:
[tex]\[ \text{Percent Yield} = \left( \frac{10 \text{ g}}{48.08 \text{ g}} \right) \times 100\% \approx 20.80\% \][/tex]

### Final Answers

1. Theoretical Yield of NaCl:
[tex]\[ \approx 48.08 \text{ grams} \][/tex]

2. Percent Yield:
[tex]\[ \approx 20.80\% \][/tex]

These answers give a detailed breakdown of the theoretical yield and percent yield calculations for the given chemical reaction.
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