In a constant volume calorimeter 3.5 g of a gas (mol.wt.28) was burnt in excess O2 at 298 K. T

step 1 We need to find energy released due to the combustion of 28 gram of a gas So first we find the e

In a constant volume calorimeter 3.5 g of a gas (mol.wt.28)...

In a constant volume calorimeter $3.5 \mathrm{~g}$ of a gas (mol.wt.28) was burnt in excess $\mathrm{O}_{2}$ at $298 \mathrm{~K}$. The increase in temperature is $0.45 \mathrm{~K}$ due to combustion. If Heat capacity of calorimeter is $2.5 \mathrm{~K} 5 / \mathrm{K}$ the value of $\Delta \mathrm{E}$ is (a) $90 \mathrm{~kJ} / \mathrm{m}$ (b) $9 \mathrm{~kJ} / \mathrm{m}$ (c) $45 \mathrm{~kJ} / \mathrm{m}$ (d) $18 \mathrm{~kJ} / \mathrm{m}$

In a constant volume calorimeter $3.5 \mathrm{~g}$ of a gas (mol.wt.28) was burnt in excess $\mathrm{O}_{2}$ at $298 \mathrm{~K}$. The increase in temperature is $0.45 \mathrm{~K}$ due to combustion. If Heat capacity of calorimeter is $2.5 \mathrm{~K} 5 / \mathrm{K}$ the value of $\Delta \mathrm{E}$ is
(a) $90 \mathrm{~kJ} / \mathrm{m}$
(b) $9 \mathrm{~kJ} / \mathrm{m}$
(c) $45 \mathrm{~kJ} / \mathrm{m}$
(d) $18 \mathrm{~kJ} / \mathrm{m}$

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Key Concepts

Constant Volume Calorimetry

Constant volume calorimetry is an experimental technique in which the reaction occurs in a container of fixed volume. Because no work is done by expansion or compression, the heat measured directly corresponds to the change in internal energy (?E) of the system.

Calorimeter Heat Capacity

The heat capacity of a calorimeter is the amount of energy required to raise its temperature by one degree. In calorimetry, this value is multiplied by the observed temperature change to determine the total energy change associated with the reaction occurring within the device.

Internal Energy Change

In the context of reactions carried out at constant volume, the energy change calculated is the change in internal energy (?E) of the system. Unlike reactions at constant pressure, no work is done due to expansion, so ?E is directly measured by the heat absorbed or released by the calorimeter.

Molar Quantities and Stoichiometry

Molar calculations involve converting a given mass of substance to moles using its molar mass. This conversion is necessary to express energy changes on a per mole basis, allowing for standardization and comparison of energetic data across different reactions.

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