The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated

Question

The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain: 2 SO_2 (g) + O_2 (g) = 2 SO_3 (g). If the equilibrium partial pressures of SO_2, O_2, and SO_3 are 0.592 atm,0.107 atm, and 0.352 atm respectively at 1000 K, what is K_p at that temperature? a. 3.30 b. 5.56 c. 0.180 d. 0.303 A vessel contains an equilibrium mixture of 0.0367 M NO,0.0673 M Br_2 and 0.149 M NOBr at 24.5 degree C. What is the value of K_p for the reaction below? 2 NO(g) + Br_2 (g) = 2 NOBr(g)? a. 245 b. 6.00 times 10^3 c. 10.0 d. 4.08 times 10^-3

Explanation / Answer

12. 2SO2 + O2 <-----> 2SO3

Equilibrium constant,Kp= p^2 SO3/(p^2 SO2 * pO2)

Kp= 0.352^2/(0.592^2 * 0.107)

= 3.30

Therefore option(a) is correct

13. 2NO + Br2 <-------> 2NOBr

Equilibrium constant Kc=[NOBr]^2 /([ NO]^2 [Br2])

Kc= 0.149^2/(0.0367^2 * 0.0673)

= 244.9

We know that KP=Kc*(RT)^dn

Where

R= gas constant=8.414 J/mol-K

T= temperature=24.5oC=24.5+273=297.5K

dn= change in number of moles= 2-(2+1)=-1

Plug the values we get Kp=0.099

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