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Oxidation of gaseous ClF by F2 yields liquid ClF3, an important fluorinating agent. Use the following thermochemical equations to calculate ΔH o rxn for the production of ClF3:
(1) 2 ClF(g) + O2(g) → Cl2O(g) + OF2(g) ΔHo = 167.5 kJ
(2) 2 F2(g) + O2(g) → 2 OF2(g) ΔHo = −43.5 kJ
(3) 2 ClF3(l) + 2 O2(g) → Cl2O(g) + 3 OF2(g) ΔHo = 394.1 kJ
calculate ΔH rxn in KJ

Respuesta :

fgschem

Answer:

ΔH = -135.05 kJ

Explanation:

(1) 2 ClF(g) + O₂(g) → Cl₂O(g) + OF₂(g)           ΔHo = 167.5 kJ

(2) 2 F₂(g) + O₂(g) → 2 OF₂(g)                         ΔHo = −43.5 kJ

(3) 2 ClF₃(l) + 2 O₂(g) → Cl₂O(g) + 3 OF₂(g)    ΔHo = 394.1 kJ

We can use Hess' Law to calculate the  ΔH of reaction:

ClF(g) + 1/2O₂(g) → 1/2Cl₂O(g) + 1/2OF₂(g)  ΔHo = 167.5  x 1/2 = 83.75 kJ

F₂(g) + 1/2O₂(g) →  OF₂(g)                             ΔHo = −43.5   x 1/2 = -21.75 kJ

1/2Cl₂O(g) + 3/2 OF₂(g) →  ClF₃(l) +  O₂(g)   ΔHo = 394.1  x -1 x 1/2 = -197.05kJ

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(4) ClF (g) + F₂ (g) → ClF₃ (l)      ΔH = 83.75 kJ-21.75 kJ-197.05kJ

ΔH = -135.05 kJ/mol

The heat of reaction for the production of ClF₃ is 135.05 kJ

From the question,

We are to calculate the heat of reaction for the formation of ClF₃

From the given information,

(1) 2ClF(g) + O₂(g) → Cl₂O(g) + OF₂(g)                      ΔHo = 167.5 kJ

(2) 2F₂(g) + O₂(g) → 2OF₂(g)                                    ΔHo = −43.5 kJ

(3) 2ClF₃(l) + 2O₂(g) → Cl₂O(g) + 3OF₂(g)                ΔHo = 394.1 kJ

Divide equation (1), (2), and (3) by 2 to get

(1) ClF(g) + ¹/₂O₂(g) → ¹/₂Cl₂O(g) + ¹/₂OF₂(g)              ΔHo = 83.75 kJ

(2) F₂(g) + ¹/₂O₂(g) → OF₂(g)                                      ΔHo = −21.75 kJ

(3) ClF₃(l) + O₂(g) → ¹/₂Cl₂O(g) + ³/₂OF₂(g)                ΔHo = 197.05 kJ

Since the product we are interested in is ClF₃,

Reverse equation (3) to get

(4) ¹/₂Cl₂O(g) + ³/₂OF₂(g) → ClF₃(l) + O₂(g)               ΔHo = -197.05 kJ

Now, add equations (1), (2), and (4)

(1) ClF(g) + ¹/₂O₂(g) → ¹/₂Cl₂O(g) + ¹/₂OF₂(g)              ΔHo = 83.75 kJ

(2) F₂(g) + ¹/₂O₂(g) → OF₂(g)                                      ΔHo = −21.75 kJ

(4) ¹/₂Cl₂O(g) + ³/₂OF₂(g) → ClF₃(l) + O₂(g)               ΔHo = -197.05 kJ

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     ClF(g) + F₂(g) → ClF₃(l)                                        ΔH rxn = 135.05 kJ

Hence, the heat of reaction for the production of ClF₃ is 135.05 kJ

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