The equilibrium constant, K_cl, of the reaction 2 NO(g) N_2(g) + O_2(g) at a tem

Question

The equilibrium constant, K_cl, of the reaction 2 NO(g) N_2(g) + O_2(g) at a temperature of 1000 K is 1.3-10^8. The equilibrium constant, K_e2, of the reaction 1/2 N_2(g) + 1/2 O_2(g) NO(g) at a temperature of 1000 K is: At 1000 K, the values of the equilibrium constants of the following two reactions have been determined: N_2O_4(g) 2 NO_2(g) K_e1 = 1.5 10^6 1/2 N_2(g) + O_2(g) NO_2(g) K_e2 = 1.2 10^-5 The following reaction is considered: N_2(g) + 2 O_2(g) N_2O_4(g) K_e3 = ? The value of K_e3 at 1000 K is: At 700 K, the values of the equilibrium constants of the following two reactions have been determined H_2(g) + I_2(g) 2 HI(g) K_c1 = 54.0 N_2(g) + 3 H_2(g) 2 NH_3(g) K_c2 = 1.04 10^-4 The following reaction is considered: 2NH_3(g) + 3 I_2(g) 6 HI(g) + N_2(g) K_c3 = ? The value of K_c3 at 900 K is:

Explanation / Answer

1)

the first reaction is

2N0 ----> N2 + 02    Kc1 = 1.3 x 10^8

now reverse the reaction

we get

N2 + 02 ---> 2 N0

when we reverse a reaction , the new equilibrium constant is the inverse of the original

so

we get

Kc = 1 / Kc1

Kc = 1/ 1.3 x 10^8

Kc = 7.69 x 10-9

now

N2 + 02 ---> N0    Kc = 7.69 x 10-9

now

multiply the reaction by 0.5 we get

0.5 N2 + 0.5 02 ---> N0

now

when we multiply a equation by a factor n , the equilibrium factor changes by the power of n

so

Kc2 = (Kc)^0.5

Kc2 = ( 7.69 x 10-9)^0.5

Kc2 = 8.77 x 10-5

so

the answer is option e ) 8.8 x 10-5

2)

considert the second reaction

0.5 N2 + 02 ---> N02

multiply the reaction with 2

we get

N2 + 202 ---> 2N02

so

Kc = (Kc2)^2

Kc = 1.44 x 10-10

now

a)N2 + 202 ----> 2N02     Kc = 1.44 x 10-10

b) N204 ----> 2N02      Kc1 = 1.5 x 10^6

c) N2 + 202 ---> N204    Kc3 = ?

now

c = a-b

so

Kc3 = Kc /Kc1

Kc3 = 1.44 x 10-10 / 1.5 x 10^6

Kc3 = 9.6 x 10-17

so

the answer is option b) 9.6 x 10-17

3)

consider the first reaction

H2 + I2 ---> 2HI   Kc1 = 54

multiply with 3

we get

3H2 + 3I2 ---> 6HI

so

Kc = (Kc1)^3

Kc = (54)^3

Kc = 157464

now

a) 3H2 + 3I2 ----> 6HI    Kc = 157464

b) N2 + 3H2 ---> 2NH3    Kc2 = 1.04 x 10-4

c) 2NH3 + 3I2 ----> 6 HI + N2   Kc3 = ?

we see that

c = a - b

so

Kc3 = Kc / Kc2

Kc3 = 157464 / 1.04 x 10-4

Kc3 = 1.514 x 10^9

so

the answer is option g) 1.51 x 10^9

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