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A sample of 0.16 g CH(4) was subjected t...

A sample of `0.16 g CH_(4)` was subjected to combustion at `27^(@)C` in a bomb calorimeter. The temperature of the calorimeter system (including water) was found to rise by `0.5^(@)C`. Calculate the heat of combustion of methane at (a) constant volume and (b) constant pressure. The thermal capacity of calorimeter system is `17.0 kJ K^(-1)` and `R = 8.314 J K^(-1) mol^(-1)`.

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To solve the problem, we will calculate the heat of combustion of methane at both constant volume and constant pressure using the provided data. ### Step 1: Write the combustion reaction of methane The balanced chemical equation for the combustion of methane (CH₄) is: \[ \text{CH}_4 + 2 \text{O}_2 \rightarrow \text{CO}_2 + 2 \text{H}_2\text{O} \] ### Step 2: Calculate the heat of combustion at constant volume (ΔE) The heat of combustion at constant volume can be calculated using the formula: ...
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