The interhalogen species iodine trichloride (IC13) may be synthesised according to the following reaction: 1₂ (s) + 3 Cl₂ (g) 2 IC13 (s) The thermodynamic data for the species are: S°(J mol¹) AH (kJ mol¹) 62.26 1₂ (g) 260.6 1₂ (s) 0 116.7 Ch₂ (g) 0 223.0 IC13 (s) -88.28 172.0 a) Calculate the Standard Gibbs Free Energy (4G) for the reaction at 25 °C. b) Is this reaction spontaneous at 25 °C? Explain your answer. c) At a given point as the reaction proceeds at 120 °C, the solution contains 0.52 g of I₂, 0.18 g of ICI, and 0.0824 mol L¹ of Cl₂. Calculate AG for the reaction under these conditions and determine in which direction the reaction will spontaneously proceed.

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Hi i am unable to solve part C from my practice exams, can I pelase have some help?

The interhalogen species iodine trichloride (IC13) may be synthesised according to the following
reaction:
1₂ (s) + 3 Cl₂ (g) → 2 IC13 (s)
The thermodynamic data for the species are:
AH
(kJ mol¹)
62.26
S°(J mol¹)
I₂ (g)
260.6
I₂ (s)
0
116.7
Cl₂ (g)
0
223.0
IC13 (s)
-88.28
172.0
a) Calculate the Standard Gibbs Free Energy (AG°) for the reaction at 25 °C.
b) Is this reaction spontaneous at 25 °C? Explain your answer.
c) At a given point as the reaction proceeds at 120 °C, the solution contains 0.52 g of 12, 0.18 g of
ICl3 and 0.0824 mol L of Cl₂2. Calculate 4G for the reaction under these conditions and determine
in which direction the reaction will spontaneously proceed.
Transcribed Image Text:The interhalogen species iodine trichloride (IC13) may be synthesised according to the following reaction: 1₂ (s) + 3 Cl₂ (g) → 2 IC13 (s) The thermodynamic data for the species are: AH (kJ mol¹) 62.26 S°(J mol¹) I₂ (g) 260.6 I₂ (s) 0 116.7 Cl₂ (g) 0 223.0 IC13 (s) -88.28 172.0 a) Calculate the Standard Gibbs Free Energy (AG°) for the reaction at 25 °C. b) Is this reaction spontaneous at 25 °C? Explain your answer. c) At a given point as the reaction proceeds at 120 °C, the solution contains 0.52 g of 12, 0.18 g of ICl3 and 0.0824 mol L of Cl₂2. Calculate 4G for the reaction under these conditions and determine in which direction the reaction will spontaneously proceed.
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