Question

The heat liberated on complete combustion of 1mole CH4 gas to CO2(g) and H2O(l) is 890kJ. Calculate the heat evolved by 2.4L of CH4 on complete combustion. (1mole of CH4 at 298K and 1atm=24L)

Answer 1

Answer:- 89 kJ.

Solution:- It asks to calculate the heat evolved by the combustion of 2.4 L of methane. From Given information, The volume of 1 mol of methane at 298 K and 1 atm pressure is 24 L. Let's calculate the moles of methane for it's 2.4 L as:

$2.4L(\frac{1mol}{24L})$  

= 0.10 mol

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

$0.10mol(\frac{890kJ}{1mol})$

= 89 kJ

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

Answer 2

Answer:

95.3 is the answer......