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  3. 1.for the reaction, pcl5(g) <-----> pcl3(g)

1.For the reaction, PCl5(g) <-----> PCl3(g) + Cl2(g)          Kp = 24.6 at 500 K calculate the equilibrium partial pressures of...

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Chemistry

1.For the reaction,

PCl5(g) <-----> PCl3(g) +Cl2(g)          Kp= 24.6 at 500 K


calculate the equilibrium partial pressures of the reactants andproducts if the initial pressures are PPCl5 =0.610 atm, PPCl3 = 0.400 atm andPCl2 = 0.000 atm.

PPCl5 = PPCl3 =PCl2 =

2.

H2O(g) + Cl2O(g) <----->2HClO(g)          Kc= 0.14 at 298.15 K


calculate the equilibrium concentrations of the reactants andproducts if the initial concentrations are [H2O(g)] =0.00482 mol L-1, [Cl2O(g)] = 0.00482 molL-1 and [HClO(g)] = 0.000 mol L-1.

[H2O(g)] = [ClO2(g)] = [HClO(g)] =

3.A flask that initially contained pure NO2 washeated to 1000 K, a temperature at which the value of Kpfor the decomposition of NO2 is 128.8.

2NO2(g) <-----> 2NO(g) + O2(g)


Given that the partial pressure of O2 at equilibriumequals 0.168 atm calculate the partial pressures of NO2and NO at equilibrium.

PNO = PNO2 =

4.The equilibrium constant Kp for thereaction,

2 SO3(g) <-------> 2 SO2(g) +O2(g)


is 8.440 at 789 °C. If a vessel at this temperature initiallycontains pure SO3 and if the partial pressure ofSO3 at equilibrium is 0.050 atm, what is the partialpressure of O2 in the flask at equilibrium?

What was the initial pressure of SO3 in theflask?

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