(A) Calculate the partial pressure (in atm) of H 2 atequilibrium, when 1.69 atm

Question

(A)
Calculate the partial pressure (in atm) of H2 atequilibrium, when 1.69 atm of H2O dissociates at 1500 Kaccording to the following chemical equilbrium:

2 H2O (g) ? 2 H2 (g) +  O2 (g) Kp = 6.21 x 10-13

If the 5% approximation is valid, use the assumption to compute thepartial pressure. Report your answer to three significant figuresin scientific notation.



(B)

Calculate the partial pressure (in atm) ofC2H6 at equilibrium, when 1.39 atm ofC2H5Cl and 1.39 atm of HCl and react at 3000K according to the following chemical equation:

C2H5Cl (g) + HCl (g) ? C2H6 (g) + Cl2 (g) Kp = 6.73 x 10-3
Report your answer to three significant figures in scientificnotation.


Thanks in advance!
2 H2O (g) ? 2 H2 (g) +  O2 (g) Kp = 6.21 x 10-13

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