Question

When 1.0 g of fructose, C₆H₁₂O₆(s), is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58 °C. If the heat capacity of the calorimeter and its contents is 9.90 kJ/°C, what is q for this combustion?

a) 9.90 kJ
b) 0.0158 kJ
c) 0.156 kJ
d) 0.099 kJ

Answer 1

To calculate the heat released (q) during the combustion of fructose in a bomb calorimeter, we multiply the heat capacity of the calorimeter by the change in temperature, resulting in 15.6 kJ.

Step-by-step explanation:

The question asks for the heat released (q) when 1.0 g of fructose, C6H12O6(s), is burned in a calorimeter and the temperature increases by 1.58 °C. The measured heat capacity of the calorimeter is 9.90 kJ/°C. To find q for the combustion, we use the formula q = mcΔT, where m is the mass of the water, c is the specific heat capacity of the water, and ΔT is the change in temperature.

However, given that we have the heat capacity of the entire calorimeter, including its contents, we can simplify the formula to q = CΔT, where C is the calorimeter's heat capacity and ΔT is the temperature change.

Using the given values:

q = (9.90 kJ/°C) x (1.58 °C)

q = 15.642 kJ, which after rounding to three significant figures becomes 15.6 kJ as the heat released during the combustion.