Problem: Part ACalculate the enthalpy change, ΔH, for the expansion of methaneCH4(g) → C(g) + 4H(g)Part BCalculate the enthalpy change, ΔH for the reverse of the formation of methane.CH4(g) → C(s) + 2 H2(g)Part CSuppose that 0.570 mol of methane CH4(g) is reacted with 0.720 mol of fluorine, F2(g), forming CF4(g) and HF (g) as sole products. Assuming that the reaction occurs at constant pressure, how much heat is released?

FREE Expert Solution

Part A) Calculate the enthalpy change, ΔH, for the expansion of methane:

We can use the following equation to solve for ΔH˚rxn:

ΔH°rxn=ΔH°f, prod-ΔH°f, react

Note that we need to multiply each ΔH˚f by the stoichiometric coefficient since ΔH˚f is in kJ/mol. 

Also, note that ΔH˚f for elements in their standard state is 0.


CH4(g) → C(g) + 4 H(g)

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Problem Details

Part A

Calculate the enthalpy change, ΔH, for the expansion of methane

CH4(g) → C(g) + 4H(g)

Part B

Calculate the enthalpy change, ΔH for the reverse of the formation of methane.

CH4(g) → C(s) + 2 H2(g)

Part C

Suppose that 0.570 mol of methane CH4(g) is reacted with 0.720 mol of fluorine, F2(g), forming CF4(g) and HF (g) as sole products. Assuming that the reaction occurs at constant pressure, how much heat is released?

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