A2.15g sample of benzene (c_6h_6) is burned in a bomb calorimeter, and the temperature rises from 22.46 degree c to 34.34 degree c. calculate the heat capacity of the bomb calorimeter. note the following thermochemical equation: c_6h_6(i) + 15/2 o_2 (g) rightarrow 6co_2 (g) + 3h_2o (g) delta h degree = -3267.5 kj

The heat capacity of the bomb calorimeter is 7.58 J/°C.

Explanation:

First, we will calculate energy released on combustion:

= enthalpy change =  -3267.5 kJ/mol

q = heat energy released

n = number of moles benzene=

q = -90.0657 kJ = -90,065.7 J

Now we  calculate the heat gained by the calorimeter let it be Q.

Q = -q= -(-90,065.7 J) = 90,065.7 J (conservation of energy)

where,

Q = heat gained by calorimeter

c = specific heat capacity of calorimeter =?

= final temperature =

= initial temperature =

Now put all the given values in the above formula, we get:

The heat capacity of the bomb calorimeter is 7.58 J/°C.

it should have an internal chamber and two thermometers sticking out of the top. the internal chamber will also be closed off from the outside.