0.16 g of methane is subjected to combustion at 27^∘ C in a bomb calorimeter system. The tempera

step 1 We are given that the thermal capacity thermal capacity of the calorie meter system is given as

0.16 g of methane is subjected to combustion at 27^∘ C in a...

0.16 g of methane is subjected to combustion at $27^{\circ} \mathrm{C}$ in a bomb calorimeter system. The temperature of the calorimeter system (including water) was found to rise by $0.5^{\circ} \mathrm{C}$. Calculate the heat of combustion of methane at constant volume. The thermal capacity of the calorimeter system is $177 \mathrm{~kJ} \mathrm{~K}^{-1}\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$ (a) $-695 \mathrm{~kJ} \mathrm{~mol}^{-1}$ (b) $-1703 \mathrm{~kJ} \mathrm{~mol}^{-1}$ (c) $-890 \mathrm{~kJ} \mathrm{~mol}^{-1}$ (d) $-885 \mathrm{~kJ} \mathrm{~mol}^{-1}$

0.16 g of methane is subjected to combustion at $27^{\circ} \mathrm{C}$ in a bomb calorimeter system. The temperature of the calorimeter system (including water) was found to rise by $0.5^{\circ} \mathrm{C}$. Calculate the heat of combustion of methane at constant volume. The thermal capacity of the calorimeter system is $177 \mathrm{~kJ} \mathrm{~K}^{-1}\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$
(a) $-695 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(b) $-1703 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(c) $-890 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(d) $-885 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Key Concepts

Molar Conversion

Converting energy changes from per experiment to a per mole basis involves using the mass of the reactant burned along with its molar mass to determine the number of moles. This molar conversion standardizes the energy release, allowing for comparisons and application to theoretical thermochemical equations.

Energy Calculation in Calorimetry

In calorimetric experiments, the energy released or absorbed by a reaction can be determined using the formula Q = C × ?T, where ?T is the change in temperature and C is the heat capacity of the calorimeter system. This calculation is fundamental in relating the measured temperature change to the reaction energy.

Bomb Calorimetry

Bomb calorimetry involves conducting reactions in a sealed, constant-volume container to accurately measure the energy released or consumed during chemical reactions. Since the process occurs at constant volume, the change in internal energy directly corresponds to the heat evolved, without the work associated with gas expansion.

Heat Capacity

Heat capacity is a measure of the amount of energy required to raise the temperature of a system by one degree. In calorimetry, the thermal capacity of the calorimeter is used to calculate the total heat absorbed, where the energy change, Q, is determined by multiplying the heat capacity by the observed temperature change.

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