Problem: Part A. Calculate the enthalpy change, delta H, for the expansion of methaneCH4(g) → C(g) + 4H(g)Part B. Calculate the enthalpy change, delta H for the reverse of the formation of methane.CH4(g) → C(s) + 2H2(g)Part C. Suppose that 0.570 mol of methane CH 4(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?Use the data below to answer the questions.

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PART A

We’re being asked to determine the standard enthalpy change (ΔH˚rxn) for the balanced reaction:


CH4(g) → C(g) + 4H(g)


Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved:

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Problem Details

Part A. Calculate the enthalpy change, delta H, for the expansion of methane

CH4(g) → C(g) + 4H(g)

Part B. Calculate the enthalpy change, delta H for the reverse of the formation of methane.

CH4(g) → C(s) + 2H2(g)

Part C. Suppose that 0.570 mol of methane CH 4(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?

Use the data below to answer the questions.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.

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Based on our data, we think this problem is relevant for Professor Arasasingham's class at UCI.