The equilibrium 2 NO(g) + Cl2(g) 2 NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (a) Calculate Kp for this reaction at 500.0 K. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.

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roseswan701Lv1

27 Apr 2020

The equilibrium 2 NO(g) + Cl₂(g) 2 NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl₂, and NOCl, respectively. (a) Calculate K_p for this reaction at 500.0 K. (b) If the vessel has a volume of 5.00 L, calculate K_c at this temperature.

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Casey DurganLv2

26 May 2020

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Related questions

The equilibrium
2NO(g)+Cl2(g)â2NOCl(g)
is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 9.70Ã10^â2 atm , 0.175 atm , and 0.27 atm for NO, Cl2, and NOCl, respectively.

Part A)

Calculate Kp for this reaction at 500.0 K.

Part B)

If the vessel has a volume of 5.00 L , calculate Kc at this temperature.

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