Answer: The heat required for the process is 4.24 kJ
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Given mass of benzene = 24.8 g
Molar mass of benzene = 78.11 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of benzene}=\frac{24.8g}{78.11g/mol}=0.318mol[/tex]
To calculate the enthalpy change of the reaction, we use the equation:
[tex]\Delta H_{rxn}=\frac{q}{n}[/tex]
where,
[tex]q[/tex] = amount of heat absorbed = ?
n = number of moles = 0.318 moles
[tex]\Delta H_{rxn}[/tex] = enthalpy change of the reaction = 30.7 kJ/mol
Putting values in above equation, we get:
[tex]30.7kJ/mol=\frac{q}{0.318mol}\\\\q=(30.7kJ/mol\times 0.318mol)=4.24kJ[/tex]
Hence, the heat required for the process is 4.24 kJ
