Question

2.67 grams of butane (C4H10) is combusted in a bomb calorimeter. The temperature increases from 25.68 C to 36.2C. What is the change in the internal energy (deltaE) in KJ/mol for the reaction if the heat capacity of the bomb calorimeter is 5.73 kJ/C?

Answer 1

The internal energy : 1310.43 kJ/mol

Further  explanation

Internal energy (ΔE) can be formulated for Calorimeter :

$\tt \Delta E=C\times.\Delta t$

C= the heat capacity of the calorimeter

Δt=36.2-25.68=10.52°C

$\tt \Delta E=5.73 kJ/^oC\times 10.52^oC=60.2796~kJ$

• mol butane(MW=58,12 g/mol)

$\tt \dfrac{2.67}{58,12 }=0.046$

• the internal energy (ΔE) in KJ/mol

$\tt \dfrac{60.2796}{0.046}=1310.43~kJ/mol$