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The combustion of 136 g of methane (ch4) in the presence of excess oxygen gas produces 353 g carbon dioxide. [ch4 + 2o2--> CO2 + 2h2o; c= 12.01 g/mol, h = 1.01 g/mol, o = 16.0 g/mol]rnwhat is the percent yield?rn0.00946rn0.026rn0.385rn0.947

Accepted Answer

Here's how to calculate the percent yield:
1. Calculate the theoretical yield:
- Find the moles of methane: 136 g CH4 / (16.04 g/mol) = 8.48 mol CH4
- Use the balanced equation to find the moles of CO2 produced: 8.48 mol CH4
(1 mol CO2 / 1 mol CH4) = 8.48 mol CO2
- Convert moles of CO2 to grams: 8.48 mol CO2
(44.01 g/mol) = 373 g CO2 (theoretical yield)
2. Calculate the percent yield:
- Percent yield = (actual yield / theoretical yield)
100%
- Percent yield = (353 g CO2 / 373 g CO2)
100% = 94.7%
Therefore, the percent yield is 0.947.

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