Sulfur oxychloride decomposes to sulfur dioxide and chlorine gases: SO_2CI_2(g)

Question

Sulfur oxychloride decomposes to sulfur dioxide and chlorine gases: SO_2CI_2(g) = SO_2(g) + CI_2(g) partial pressures: 1.88 atm 0.84 atm 0.27 atm, a. At this equilibrium condition, calculate K_p b. If the partial pressure of chlorine gas is increased to 0.68 atm. what will be the value of Q_ ? c. Considering this Q_, in which direction will the reaction proceed, and why? Write the products and solubility product expressions for dissolution of the following two solids: a. Ba(OH)_2(g) b. Ag_2CrO_4(g)

Explanation / Answer

6)a)

the equilibrium is SO2Cl2 (g ) <-----> SO2 (g) + Cl2(g)

Kp = PSO2 xPCl2 /PSO2CL2

Given PSO2Cl2 = 1.88 atm

PSo2 =0.84 atm

PCl2 = 0.27 atm at equilibrium

Thus Kp = 0.84x0.27 /1.88

= 0.1206 atm

b) when PCl2 = 0.68 atm,

Qc = 0.84x 0.68/1.88

= 0.3038

As Qc > Kc the reaction proceeds in ackward direction.

7) a)

Ba(OH)2 (s) <------> Ba+2 (aq) + 2OH- (aq)

Ksp = [Ba+2][OH-]2

b) Ag2CrO4 (s) <------. )> 2Ag+ (aq) + CrO4-2(aq)

Ksp = [Ag+]2[crO4-2]

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