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Anonymous

Oct 29, 2024

In an analysis of interhalogen reactivity, 0.440 mol of ICl was placed in a 5.00−L flask, where it decomposed at a high T: 2 ICl(g)

In an analysis of interhalogen reactivity, 0.440 mol of ICl was placed in a 5.00 L flask, where it decomposed at a high temperature according to the following equilibrium reaction:

2 ICl(g) ⇌ I2(g) + Cl2(g).

Given that the equilibrium constant (Kc) at this temperature is 0.110, calculate the equilibrium concentrations of I2, Cl2, and ICl.

Please provide your answers in molarity (M) for the following: [I2]eq: [Cl2]eq: [ICl]eq:

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3 Answers

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Anonymous

Feb 05, 2025

[I2] = [Cl2] = 0.0176 M[ICl]  = 0.0528 MExplanation:Step 1: Data given Number of moles ICI = 0.440 molesVolume = 5.00 LKc = 0.110Step 2: The balanced equation2 ICl(g) ⇌ I2(g) + Cl2(g) Step 3: The initial concentrations[[ICl] = 0.440 moles/5.00 L = 0.088 M[I2[ = 0M[Cl2] = 0MStep 4: The concentrations at the equilibrium[[ICl] =(0.088 - 2x) M[I2[ =xM[Cl2] = xMStep 5: Define KcKc =0.110 = [I2][Cl2] / [ICl]²  0.110 = x² / (0.088 - 2x)²0.332 = x(0.088 - 2x)x = 0.332 *(0.088 - 2x)x = 0.029216 - 0.664x1.664x = 0.029216x = 0.0176[I2] = [Cl2] = 0.0176 M[ICl] = 0.088  - 2(0.0176 )  = 0.0528 M
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Chemistry

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Chemistry Equilibrium Reactivity

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