Question

a. A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter.

In the laboratory a student burns a 0.532-g sample of nonanedioic acid (C₉H₁₆O₄) in a bomb calorimeter containing 1050. g of water. The temperature increases from 25.30 °C to 27.90 °C. The heat capacity of water is 4.184 J g^-1°C^-1.

The molar heat of combustion is −4774 kJ per mole of nonanedioic acid.

• C₉H₁₆O₄(s) + 11 O₂(g) --> 9 CO₂(g) + 8 H₂O(l) + Energy

Calculate the heat capacity of the calorimeter.

heat capacity of calorimeter = _____ J/°C

b.

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

In an experiment, a 0.4501 g sample of 2-naphthylacetic acid (C₁₂H₁₀O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.274×10³ g of water. During the combustion the temperature increases from 27.81 to 30.13 °C. The heat capacity of water is 4.184 J g^-1°C^-1.

The heat capacity of the calorimeter was determined in a previous experiment to be 877.1 J/°C.

Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 2-naphthylacetic acid based on these data.

C₁₂H₁₀O₂(s) + (27/2) O₂(g) --> 5 H₂O(l) + 12 CO₂(g) + Energy

Molar Heat of Combustion = ____ kJ/mol

Answer 1