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].
