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Hitman42 [59]
3 years ago
5

Consider the following balanced equation for the following reaction:

Chemistry
1 answer:
balandron [24]3 years ago
8 0

<u>Answer:</u> The amount of carbon dioxide formed in the reaction is 47.48 grams

<u>Explanation:</u>

For the given chemical equation:

15O_2(g)+2C_6H_5COOH(aq.)\rightarrow 14CO_2(g)+6H_2O(l)

To calculate the actual yield of carbon dioxide, we use the equation:

\%\text{ yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\times 100

Percentage yield of carbon dioxide = 83 %

Theoretical yield of carbon dioxide = 1.30 moles

Putting values in above equation, we get:

83=\frac{\text{Actual yield of carbon dioxide}}{1.30moles}\times 100\\\\\text{Actual yield of carbon dioxide}=\frac{1.30\times 83}{100}=1.079moles

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 1.079 moles

Putting values in above equation, we get:

1.079mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(1.079mol\times 44g/mol)=47.48g

Hence, the amount of carbon dioxide formed in the reaction is 47.48 grams

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