Question

Q) The heat evolved when 4.8g of methane is burnt in excess of O2 is [∆cH°(CH4) = - 880KJ mol-1]
A) -26.4 KJ
B) -264 KJ
C) -2.64 KJ
D) -2640 KJ

plz ans fast..​

Answer 1

Answer:

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Explanation:

Looking at it is very much easier than it was in my previous post

Answer 2

The correct option to the following question is (b).

Given: mass of methane = 4.8g

           enthalpy of combustion of methane = - 880KJ mole⁻¹

To find:  heat evolved when 4.8g methane is burnt

Solution: The balanced reaction which occurs when methane is burned is -

CH₄ + 2O₂ → CO₂ + 2H₂O

As one mole of methane reacts with two moles of oxygen to form one mole of carbon dioxide and two moles of water.

One mole produces 880KJ mol⁻¹

The molecular mass of methane = 16

Mole of methane = 4.8/16 = 0.3

O.3 mole of methane produces 880 × 0.3 KJ mol⁻¹ = 264 KJ

Therefore, 4.8g of methane produces -264 KJ of energy when burnt in excess of oxygen.

• The Heat of combustion is the heat energy released when one mole of the compound is burnt.