Butane, C4H10 has a standard enthalpy of combustion = - 2881 kJ/mol

For part b, the enthalpy change when 4.000 g of butane is completely burned was - 198.3 kJ

Assuming the specific heat capacity of water to be 4.200 J/g K, and that in such a reaction only 63.15% of the energy generated is actually transferred to the water, calculate the change in temperature of 2.000kg of water that is heated by burning the butane in part b above.

14.91 K.

Explanation:

To solve this problem, we can use the following relation:

Q = m. c.ΔT,

where, Q is the amount of heat transferred to water.

m is the mass of the amount of water (m = 2.0 kg = 2000.0 g).

c is the specific heat capacity of water (c = 4.2 J/g. K).

ΔT is the change in temperature due to the transfer of butane burning.

To determine Q that to be used in calculation:

Q from 4.000 g of butane is completely burned is - 198.3 kJ = 198300 J.

The negative sign symbolizes the the enthalpy change is exothermic, which means that the energy is released.

Note that only 63.15% of the energy generated is actually transferred to the water.

∴ Q (the amount of heat transferred to water) = (198300 J) (0.6315) = 125226.45 J.

Now, we can obtain the change in temperature:

∴ ΔT = Q/m. c. = (125226.45 J) / (2000.0 g) (4.2 J/g. K) = 14.9079 K ≅ 14.91 K.

This means that the temperature is increased by 14.91 K.