The following equilibrium exists in a closed container: N2(g) + O2(g) <---> 2 NO

Question

The following equilibrium exists in a closed
container:
N2(g) + O2(g) <---> 2 NO(g)
If the partial pressures of N2, O2 and NO
at equilibrium are 1.5 atm, 2.5 atm and
0.75 atm respectively, what is the equilbrium
constants? 1. K = 5
2. K = 0.15
3. K = 0.2
4. K = 6.67 The following equilibrium exists in a closed
container:
N2(g) + O2(g) <---> 2 NO(g)
If the partial pressures of N2, O2 and NO
at equilibrium are 1.5 atm, 2.5 atm and
0.75 atm respectively, what is the equilbrium
constants? 1. K = 5
2. K = 0.15
3. K = 0.2
4. K = 6.67 1. K = 5
2. K = 0.15
3. K = 0.2
4. K = 6.67

Explanation / Answer

The equillibrium constant can be predicted for the givenreaction is                                                     Kp = PNO2 /PN2*PO2 In the given problem we have the equillibrium partialpressues, by putting these values in the above equation -                                                       Kp= (0.75)2 / 1.5*2.5                                                             =0.15 Hence 2) is the correct answer. In the given problem we have the equillibrium partialpressues, by putting these values in the above equation -                                                       Kp= (0.75)2 / 1.5*2.5                                                             =0.15 Hence 2) is the correct answer.

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