8. Thermochemistry

H₂O (l) → H₂O (g); ΔH = +44.0 kJ/mol

A sample of 0.562 g of carbon is burned in oxygen in a bomb calorimeter, producing carbon dioxide. assume both the reactants and products are under standard state conditions, and that the heat released is directly proportional to the enthalpy of combustion of graphite. The temperature of the calorimeter increases from 26.74 °C to 27.93 °C. What is the heat capacity of the calorimeter and its contents?

When a 0.740-g sample of trinitrotoluene (tnt), C₇H₅N₂O₆, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter is 534 J/°C, and it contains 675 ml of water. How much heat was produced by the combustion of the tnt sample?

Calculate the heat capacity of a calorimeter if the combustion of 5.000g of benzoic acid

Calculate the heat capacity of the calorimeter if the combustion of 5.000g of benzoic acid

Compare the calorimeter that you built to a bomb calorimeter. How are they similar and different?

What is the approximate energy density (in mj/kg) of olive oil?

Glycerol (also called glycerine), C₃H₈O₃(𝑙), is a viscous, sweet-tasting liquid used in a variety of food and personal care products. Under constant-volume conditions, the combustion of 1.000 mol of glycerol releases 1653 kJ of heat to the surroundings. A 2.850-g sample of glycerol is burned in a bomb calorimeter. The temperature of the calorimeter increases from 22.11 to 27.42°C.

a. Write a balanced equation for the combustion reaction, assuming the products are CO₂(𝑔) and H₂O(𝑙).

b. What is the total heat capacity of the calorimeter?

c. If the size of the glucose sample had been 4.000 g, what would the temperature change of the calorimeter have been?

d. Which of the following values about the combustion of glycerol under constant volume is or are correct:

i.Δ𝐻=−1653 kJ/mol;

ii. Δ𝐸=−1653 kJ/mol;

iii. 𝑞𝑣=−1653 kJ/mol?