Question

3.51 g
previous answers
correct
correct answer is shown. your answer 3.50 g was either rounded differently or used a different number of significant figures than required for this part.
because pb(no₃)₂ is the limiting reactant, the theoretical yield is the mass of pbcl₂ produced from complete consumption of pb(no₃)₂:
theoretical yield = mol pbcl₂ × molar mass of pbcl₂ = 1.26×10⁻² mol pbcl₂ × 278.106 g pbcl₂ / 1 mol pbcl₂ = 3.51 g pbcl₂
part c
determine the percent yield.
express your answer to three significant figures.
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Explanation:

Step1: Recall percent - yield formula

Percent yield = $\frac{\text{actual yield}}{\text{theoretical yield}}\times100\%$

Step2: Assume actual yield value

Let's assume the actual yield value is given (not shown in the provided text, but we know theoretical yield = 3.51 g). For the sake of demonstration, if the actual yield is 3.00 g.
Percent yield = $\frac{3.00\ g}{3.51\ g}\times100\%$

Step3: Calculate percent yield

Percent yield = $\frac{3.00}{3.51}\times100\% \approx 85.5\%$

Answer:

85.5% (assuming actual yield of 3.00 g. You need to substitute the actual yield value given in the full - context problem to get the accurate answer)