Solution Found!
Answer: Using the following information and the fact that
Chapter 9, Problem 88P(choose chapter or problem)
Using the following information and the fact that the average C—H bond enthalpy is 414 kJ/mol, estimate the standard enthalpy of formation of methane \(\mathrm {(CH_4)}\).
\(\mathrm{C}(s) \longrightarrow \mathrm{C}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=716 \mathrm{~kJ} / \mathrm{mol}\)
\(2 \mathrm{H}_{2}(g) \longrightarrow 4 \mathrm{H}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=872.8 \mathrm{~kJ} / \mathrm{mol}\)
Questions & Answers
QUESTION:
Using the following information and the fact that the average C—H bond enthalpy is 414 kJ/mol, estimate the standard enthalpy of formation of methane \(\mathrm {(CH_4)}\).
\(\mathrm{C}(s) \longrightarrow \mathrm{C}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=716 \mathrm{~kJ} / \mathrm{mol}\)
\(2 \mathrm{H}_{2}(g) \longrightarrow 4 \mathrm{H}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=872.8 \mathrm{~kJ} / \mathrm{mol}\)
ANSWER:Step 1 of 4
Here, we will find out the standard enthalpy formation of methane.
Standard enthalpy of formation:
The enthalpy change when 1 mole of a compound produced from its elements under standard conditions.
It is indicated by the