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??3:43 cvg.cengagenow.com ???? Bing Google Yahoo ???? Pad ?+ Write The Cell Notat ????-???? ???????? CengageBrain- My...OWLv2 | Online t.. BREAK At 25°C, gascous SO2Cl2 decomposes to SO2(9) and Cl2(9) to the extent that 17.0% of the original so,C12 (by moles) has decomposed to reach equilibrium. The total pressure (at equilibrium) is 0.480 atm. Calculate the value of Kp for this system. Question 1 1 pt Question 2 1 pt Question 3 Question 4 Question 5 1 pt Submit Answer Try Another Version 1 pt 1 pt 1 pt Question 6 9 item attempts remaining Question Question 8 Question 9 Question 10 1 pt 1 pt 1 pt Question 11 Question 12 Question 13 Question 14 Question 15 1 pt 1 pt Progress: 0/16 items Due Apr 8 at 11:55 PMM Previous Next Email Instructor Save and Exit Cengage Learning Cengage Technical S

Explanation / Answer

SO2Cl2(g) = SO2(g) + Cl2(g)

let x = initial pressure of SO2Cl2

I: x 0 0
C: -0.17x +0.17x +0.17x
E: x-0.17x +0.17x +0.17x

Pressure Total @ Equilibrium = x-0.17x+0.17x+0.17x
0.48 atm = x+0.17x
0.48 atm = 1.17x
x = 0.48/1.17 = 0.410atm

Now, plug in x to find the partial pressures of the gases @ equilibrium:

P(SO2Cl2) = 0.410-0.17(0.410) = 0.410-0.0697 = 0.340atm
P(SO2) = 0.17(0.410) = 0.0697atm
P(Cl2) = 0.17(0.410) = 0.0697atm

Now solve for Kp:

Kp = (0.0697)^2/(0.340) = 1.43x10^-2

Note: keep in mind that in this problem you can consider moles of SO2Cl2 gas equals pressure of SO2Cl2 gas by the relationship of the mole fraction: npartial/ntotal = Ppartial/Ptotal

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