Balanced reaction: CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g)
ΔH˚rxn = –1952.2 kJ/mol
Find the limiting reactant:
HF from CH4:
molar mass CH4 = 16.042 g/mol
moles HF = 0.860 mol HF
HF from F2:
Suppose that 3.45 g CH4(g) reacts with 1.22 g F2(g), forming CF4(g) and HF(g) as sole products. If the reaction occurs at constant pressure, what amount of heat is evolved?
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