4. Suppose that HCl is transferred to a reaction vessel at a pressure of 0.22 atm and is allowed to form H2 and O2 at 298. K; at this temp. Kp 3.2 x 1034 for the reaction - 2 HCl(g) H2(g) + Cl2(g) Calculate the partial pressures of the gases in the equilibrium mixture. (Ans: PHC 0.22 atm ; PH2 3.9 x 1018 atm; PN20-3.9 X 1018 atm)

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Please work out question #4 completely. I need to see the steps and how the equations are set up.

4. Suppose that HCl is transferred to a reaction vessel at a pressure of 0.22 atm and is allowed to form
H2 and O2 at 298. K; at this temp. Kp 3.2 x 1034 for the reaction
-
2 HCl(g) H2(g) + Cl2(g)
Calculate the partial pressures of the gases in the equilibrium mixture.
(Ans: PHC 0.22 atm ; PH2 3.9 x 1018 atm; PN20-3.9 X 1018 atm)
Transcribed Image Text:4. Suppose that HCl is transferred to a reaction vessel at a pressure of 0.22 atm and is allowed to form H2 and O2 at 298. K; at this temp. Kp 3.2 x 1034 for the reaction - 2 HCl(g) H2(g) + Cl2(g) Calculate the partial pressures of the gases in the equilibrium mixture. (Ans: PHC 0.22 atm ; PH2 3.9 x 1018 atm; PN20-3.9 X 1018 atm)
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