0.16g of methane when burnt raises the temperature of 100g of water by 40°C. What is the of combustion of methane when if the heat capacity of water is 4.2 Jg-1°C-1?
(CH4 = 16)
a
1,160 kJ mol-1
b
1,180 kJ mol-1
c
1,560 kJ mol-1
d
1,600kJ mol-1
e
1,680 kJ mol-1
Explanation
Correct Option
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Discussions (19)
Toclay
5 years ago
Let me give u a quicker clue in case u might see in in jamb
Add ur MCO of water*molar mass of methane /mass of methane
Answer must be in kilojoules not joules then divide by 1000
Then u get ur answer
kored
2 years ago
I think the formula for combustion they used here is Combustion=Heat energy/mole
H=mc∆temperature: m=100, c=4.2, temp=40
mole= mass/molar mass=0.16/16=0.01
= 100*4.2*40/0.01
=1,680,000 j/mol converted to kj is 1,680kj
