Final answer:
The change in enthalpy for the oxidation of liquid benzene can be calculated using the equation ΔH = q / n. By substituting the given values into the equation, we can find that the heat released for the combustion of the benzene sample is 31.4 kJ.
Step-by-step explanation:
The change in enthalpy, ΔH, for the oxidation of liquid benzene can be calculated using the equation:
ΔH = q / n
Where q is the heat released or absorbed by the reaction and n is the number of moles of the substance being oxidized.
In this case, the change in enthalpy is given as -3728 kJ and the reaction is taking place at constant pressure. To find the heat released, we need to calculate the number of moles of benzene being oxidized.
Using the equation q = mcΔT, where q is the heat absorbed by the calorimeter, m is the mass of the benzene sample, c is the heat capacity of the calorimeter, and ΔT is the change in temperature, we can find the heat released.
In the provided example, when 0.963 g of benzene is burned, the temperature of the calorimeter increases by 8.39 °C. The bomb calorimeter has a heat capacity of 784 J/°C and is submerged in 925 mL of water. By substituting the given values into the equation, we can find that the heat released for the combustion of the benzene sample is 31.4 kJ.