Part A) Calculate the enthalpy change, ΔH, for the expansion of methane:
We can use the following equation to solve for ΔH˚rxn:
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)
Calculate the enthalpy change, ΔH, for the expansion of methane
CH4(g) → C(g) + 4H(g)
Calculate the enthalpy change, ΔH for the reverse of the formation of methane.
CH4(g) → C(s) + 2 H2(g)
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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