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A chemical reaction is carried out in a bomb calorimeter. The temperature of the calorimeter increases from $\mathrm{25^{\circ} \mathrm{C}\: to \: 30^{\circ} \mathrm{C}}$ upon the reaction. The heat capacity of the calorimeter (including the water) is $\mathrm{500 \mathrm{~J} /{ }^{\circ} \mathrm{C}}$ . Calculate the heat released $\mathrm{(\Delta H)}$ by the reaction.

Option: 1
$2500 \mathrm{~J}$

Option: 2
$1600 \mathrm{~J}$

Option: 3
$1340\mathrm{~J}$

Option: 4
$1200 \mathrm{~J}$

Answers (1)

best_answer

Given data:

Initial temperature $\mathrm{\left(T_i\right)=25^{\circ} \mathrm{C}=298 \mathrm{~K}}$

Final temperature $\mathrm{\left(T_f\right)=30^{\circ} \mathrm{C}=303 \mathrm{~K}}$

Heat capacity of calorimeter $\mathrm{(C)=500 \quad \mathrm{~J} /{ }^{\circ} \mathrm{C}}$

The heat released $\mathrm{(\Delta H)}$ by the reaction can be calculated using the equation:

$\mathrm{ \Delta H=C \cdot \Delta T }$

Substitute the values and calculate $\mathrm{\Delta H:}$

$\mathrm{ \Delta H=500 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot(303 \mathrm{~K}-298 \mathrm{~K})=2500 \mathrm{~J} }$

Therefore, the heat released $\mathrm{ (\Delta H) }$ by the reaction is $\mathrm{ 2500 \mathrm{~J} }$ .

So, correct option is 1.

Posted by

shivangi.bhatnagar

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