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Globokim8

Answered question

2021-10-03

What is the standart heat of formation of methane, ∆HfCH4(g), as calculate above?

Answer & Explanation

okomgcae

Skilled2021-10-04Added 93 answers

Given that $∆ H r x n = - 889.1 k J$ and the values for $∆ H f$ for water and carbon dioxide, we can use Hess's Law to back-calculate $∆ H f$ for methane. That is,
$∆ H r x n = ∆ H f products - ∆ H f$ reactants
$- 889.1 = [2 (∆ H f H 20) + ∆ H f C O 2] - [∆ H f C H 4 + ∆ H f O 2]$
Since oxygen is being used to combust the methane, we can say that the ∆Hf for oxygen is absorbed into the ∆Hf for methane. Thus, our equation becomes
$- 889.1 = [2 (- 285.8) - 393.3] - [∆ H f C H 4]$
$- 889.1 = - 964.9 - [∆ H f C H 4]$
$75.8 = - [∆ H f C H 4]$
$∆ H f C H 4$ = - 75.8 kJ/mol

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