This is an incomplete question, here is a complete question.
A 6.55 g sample of aniline [tex](C_6H_5NH_2)[/tex] molar mass = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter.
[tex]4C_6H_5NH_2(l)+35O_2(g)\rightarrow 24CO_2(g)+14H_2O(g)+4NO_2(g)[/tex]
ΔH°rxn = -1.28 × 10⁴ kJ
Answer : The heat capacity of the calorimeter is, [tex]6.84kJ/^oC[/tex]
Explanation :
First we have to calculate the moles of aniline.
[tex]\text{Moles of aniline}=\frac{\text{Mass of aniline}}{\text{Molar mass of aniline}}[/tex]
[tex]\text{Moles of aniline}=\frac{6.55g}{93.13g/mol}[/tex]
[tex]\text{Moles of aniline}=0.0703mol[/tex]
Now we have to calculate the heat releases.
As, 4 mole of aniline on combustion to releases heat = [tex]1.28\times 10^4kJ[/tex]
So, 0.0703 mole of aniline on combustion to releases heat = [tex]\frac{0.0703}{4}\times 1.28\times 10^4kJ=224.96kJ[/tex]
Now we have to calculate the heat capacity of the calorimeter.
[tex]\text{Heat capacity of the calorimeter}=\frac{\text{Heat releases}}{\text{Change in temperature}}[/tex]
[tex]\text{Heat capacity of the calorimeter}=\frac{224.96kJ}{32.9^oC}[/tex]
[tex]\text{Heat capacity of the calorimeter}=6.84kJ/^oC[/tex]
Thus, the heat capacity of the calorimeter is, [tex]6.84kJ/^oC[/tex]
