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The bomb calorimeter is used to find the(1) heat of combustion(2) heat of neutralizution(3) heat of solution(4) heat of dilution
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A bomb calorimeter is a type of constant-volume calorimeter used in measuring the heat of combustion of a particular reaction. Show more…
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Bomb calorimeter is used to determine the heat of reaction at (1) constant pressure (2) constant volume (3) $298 \mathrm{~K}$ (4) $373 \mathrm{~K}$
Before a bomb calorimeter is used, it must first be calibrated and the calorimeter constant must be experimentally determined. Typically, standard compounds with well-known heat of combustion values are used to calibrate the bomb calorimeter. For example, benzoic acid (MW = 122.12 g mol-1) has a heat of combustion of -3227 kJ mol-1 and is commonly used to determine the calorimeter constant. 1.8 g of benzoic acid is burned in the calorimeter, which contains 1 kg of water, and the temperature of the water (specific heat capacity = 4.184 J g-1 °C-1) is observed to increase by +8.6 °C. Based on this information, calculate the calorimeter constant (in units of J °C-1). Report your answer to the nearest integer.
An alternative approach to bomb calorimetry is to establish the heat capacity of the calorimeter, exclusive of the water it contains. The heat absorbed by the water and by the rest of the calorimeter must be calculated separately and then added together. A bomb calorimeter assembly containing $983.5 \mathrm{g}$ water is calibrated by the combustion of $1.354 \mathrm{g}$ anthracene. The temperature of the calorimeter rises from 24.87 to $35.63^{\circ} \mathrm{C} .$ When $1.053 \mathrm{g}$ citric acid is burned in the same assembly, but with 968.6 g water, the temperature increases from 25.01 to $27.19^{\circ} \mathrm{C}$. The heat of combustion of anthracene, $\mathrm{C}_{14} \mathrm{H}_{10}(\mathrm{s}),$ is $-7067 \mathrm{kJ} / \mathrm{mol}$ $\mathrm{C}_{14} \mathrm{H}_{10} .$ What is the heat of combustion of citric acid, $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7},$ expressed in $\mathrm{kJ} / \mathrm{mol} ?$
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