Answer:
68.95
Step-by-step explanation:
To calculate the percent yield of arsenic, we need to use the actual yield and the theoretical yield of arsenic. The theoretical yield is the maximum amount of arsenic that could be produced from 92g of carbon, assuming complete conversion of the carbon to arsenic. The actual yield is the amount of arsenic that was actually produced in the reaction.
From the balanced chemical equation for the reaction, we know that the molar ratio of carbon to arsenic is 3:1. That means that 92g of carbon should produce:
(92 g C) / (12.01 g/mol C) * (1 mol As / 3 mol C) * (74.92 g/mol As) = 616.39 g of arsenic (theoretical yield)
However, the actual yield was 425g of arsenic.
To calculate the percent yield, we use the following formula:
percent yield = (actual yield / theoretical yield) x 100%
Plugging in the values, we get:
percent yield = (425 g / 616.39 g) x 100% ≈ 68.95%
Therefore, the percent yield of arsenic is approximately 68.95%.