Question

The heat liberated on complete combustion of 1 mole of ${CH}_4$ gas to ${CO}_2\left(g\right)$ and ${HO}_2\left(l\right)$ is 890 KJ. Calculate the heat evolved by 2.4 L of ${CH}_4$ on complete combustion.

• A. 95.3 KJ
• B. 8900 KJ
• C. 89 KJ
• D. 8.9 KJ

Answer 1

Answer: (C)

89 KJ

Given

The volume of $!mol$ of methane at $298K$ and $1atm$ pressure is $24L$. Let's calculate the moles of methane for it's $2.4L$ as

$=2.4\left(\frac{1mole}{24L}\right)$

$=0.10mol$

Now, it says that combustion of $1mol$ of methane generates $890J$ of heat. We could calculate the heat generated by the combustion of $0.10moles$ of methane as:

$=0.10mol\left(\frac{890kJ}{1mole}\right)$

$=89kJ$

Therefore, 89kJ of heat will be evolved by the combustion of 2.4L of methane