Define reaction quotient. How does from equilibrium constant? Outline the steps

Question

Define reaction quotient. How does from equilibrium constant? Outline the steps for calculating the reacting species in an equilibrium reaction. equilibrium constant K_P for the reaction 2SO_2(g) + O_2(g) 2SO_3(g) is 5.60 times 10^4 at 350degreeC. The initial pressures of D02 and O2 in a mixture are 0.350 atm and 0.762 atm, respectively, at 350degreeC. When the mixture equilibrates, is the total pressure less than or greater than the sum of the initial pressures (1.112 atm)? For the synthesis of ammonia N_2 (g) + 3H_2(g) 2NH_3(g) the equilibrium constant at 375 degree C is 1.2. Starting with [H_2]_0 = 0.76 [N_2]_0 = 0.60 M. and [NH_3]_0 = 0.48 M, which gases will have increased in concentration and which will have decreased in concentration when the mixture comes to equilibrium? For the reaction H_2(g) + CO_2 (g) H_2O(g) + C(g) at 700 degree C. K_c = 0.534. Calculate the number of moles of H_2 that are present at equilibrium if a mixture of 0.300 mole of CO and 0.300 mole of H_2O is heated to 700 degree C in a 10.0-L container. At 1000 K, a sample lot pure NO_2 gas decomposes: 2NO_2(g) 2NO(g) + O_2(g)

Explanation / Answer

14.40

For the synhtesis of ammonia fron N2 and H2 gas,

K = [NH3]^2/[N2][H2]^3

with,

[N2] = 0.60 M

[H2] = 0.76 M

[NH3] = 0.48 M

we get,

Kc = (0.48)^2/(0.60)(0.76)^3 = 0.87

At equilibrium, Kc = 1.2

So to reach equilibrium Kc has to go from 0.87 to 1.2,

[N2] and [H2] concentration would reduce and [NH3] concentration would increase.

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