Given the following thermochemical equation for the combustion of methane gas: CH4 (9) + 2O2 (g)...

Question

Question

Given the following thermochemical equation for the combustion of methane gas: CH4 (9) + 2O2 (g) → CO2 (g) + 2H20 (1) AH = -8

Answer 1

Answer #1

given the reaction is

CH₄(g) +2O₂(g) <===> CO₂(g) + 2H₂O(l) , ∆H = -890 kJ

from the above reaction 890 kJ energy produce 1 mole of CH4 .

now we convert moles into gram.

i.e.

890 kJ energy produce => 16 g CH₄

1 kJ energy produce => 16×1/890 g CH₄

132 kJ energy produce => 16×132/890 g CH₄

= 2.373 g of CH₄

therefore, 2.373 g of methane is required to produce 132kJ of energy.

Answer 2

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