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Solid sodium reacts with fluorine gas. The theoretical yield of the reaction is 28.2 g NaF. If 25.9 g NaF were recovered after the reaction, what is the percent yield for the reaction?

[tex]\[
2 \text{Na} + \text{F}_2 \rightarrow 2 \text{NaF}
\][/tex]

Percent yield: [tex]\[ ?\% \][/tex]



Answer :

GinnyAnswer
Sure, let's work through this step-by-step to find the percent yield of the reaction [tex]\( 2 Na + F_2 \rightarrow 2 NaF \)[/tex].

### Step 1: Identify Key Information

1. Theoretical yield: This is the amount of product that would be formed if the reaction went perfectly with no losses. The theoretical yield given is [tex]\( 28.2 \)[/tex] grams of [tex]\( NaF \)[/tex].

2. Actual yield: This is the amount of product that was actually recovered from the reaction. The actual yield given is [tex]\( 25.9 \)[/tex] grams of [tex]\( NaF \)[/tex].

### Step 2: Understand the Percent Yield Formula

The percent yield of a reaction can be calculated using the following formula:

[tex]\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \% \][/tex]

### Step 3: Plug in the Values

Let's substitute the given values into the percent yield formula:

1. Actual yield = [tex]\( 25.9 \)[/tex] grams
2. Theoretical yield = [tex]\( 28.2 \)[/tex] grams

[tex]\[ \text{Percent Yield} = \left( \frac{25.9}{28.2} \right) \times 100 \% \][/tex]

### Step 4: Solve the Equation

When we divide the actual yield by the theoretical yield:

[tex]\[ \frac{25.9}{28.2} \approx 0.9184397163120566 \][/tex]

Now, multiply this result by 100 to convert it to a percentage:

[tex]\[ 0.9184397163120566 \times 100 \approx 91.844 \% \][/tex]

### Step 5: State the Final Result

Therefore, the percent yield of the reaction is approximately [tex]\( 91.84 \% \)[/tex].

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