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  • A chemical reaction takes place in a bomb calorimeter. The calorimeter is surrounded by a water bath, and the temperature of the water bath increases from <img alt="\mathrm{20^{\circ} \mathrm{C} \:

A chemical reaction takes place in a bomb calorimeter. The calorimeter is surrounded by a water bath, and the temperature of the water bath increases from \mathrm{20^{\circ} \mathrm{C} \: to \: 22^{\circ} \mathrm{C}} upon the reaction. The heat capacity of the water bath is \mathrm{1500 \mathrm{~J} /{ }^{\circ} \mathrm{C}}. Calculate the heat released \mathrm{(\Delta H)} by the reaction.
 

Option: 1

1200 \mathrm{~J}


 


Option: 2

3400 \mathrm{~J}
 


Option: 3

2400 \mathrm{~J}
 


Option: 4

3000 \mathrm{~J}


Answers (1)

best_answer

Given data:

Initial temperature \mathrm{\left(T_i\right)=20^{\circ} \mathrm{C}=293 \mathrm{~K}}

Final temperature \mathrm{\left(T_f\right)=22^{\circ} \mathrm{C}=295 \mathrm{~K}}

Heat capacity of water bath \mathrm{(C)=1500 \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=1500 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot(295 \mathrm{~K}-293 \mathrm{~K})=3000 \mathrm{~J} }

Therefore, the heat released \mathrm{(\Delta H)} by the reaction is \mathrm{3000 \mathrm{~J}}.

So, the correct option is 4.

Posted by

Kshitij

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