How much heat is absorbed in the process of making 0.913 mol of CF₄ from the following reaction? C (s) + 2 F₂ (g) → CF₄ (g) ∆H° = 141.3 kJ/mol

Question

How much heat is absorbed in the process of making 0.913 mol of CF₄ from the following reaction?  C (s) + 2 F₂ (g) → CF₄ (g) ∆H° = 141.3 kJ/mol

J.R. S. · Accepted Answer

C(s) + 2F2(g) ==> CF4(g) ∆H = 141.3 kJ/mole

From this balanced equation we know that to make 1 mole of CF4 requires 141.3 kJ of energy.

Thus, to produce 0.913 moles of CF4 will take slightly less than that amount of energy.

141.3 kJ/mole x 0.913 moles = 129 kJ

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