When 6.0 g of graphite reacts with dihydroge | vedclass

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Question

(B) The chemical equation for the formation of methane is: $C_{(s)} + 2H_{2(g)} \longrightarrow CH_{4(g)}$
The molar mass of graphite $(C)$ is $12.0

Vedclass · Accepted Answer

$-74.8 \ kJ \ mol^{-1}$

Vedclass · Answer

(B) The chemical equation for the formation of methane is: $C_{(s)} + 2H_{2(g)} \longrightarrow CH_{4(g)}$
The molar mass of graphite $(C)$ is $12.0 \ g \ mol^{-1}$.
Given that $6.0 \ g$ of graphite releases $37.4 \ kJ$ of heat,the enthalpy change $(\Delta H)$ for this amount is $-37.4 \ kJ$.
To find the standard enthalpy of formation $(\Delta H_f^{\circ})$,we calculate the heat released for $1 \ mol$ $(12.0 \ g)$ of graphite:
$\Delta H_f^{\circ} = \frac{-37.4 \ kJ}{6.0 \ g} 	imes 12.0 \ g \ mol^{-1} = -74.8 \ kJ \ mol^{-1}$.

When $6.0 \ g$ of graphite reacts with dihydrogen to give methane gas,$37.4 \ kJ$ of heat is liberated. What is the standard enthalpy of formation of $CH_{4(g)}$?

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