The gas constant R is 8.314 J middot mol^-1-K^-1 The equilibrium expression for
ID: 974576 • Letter: T
Question
The gas constant R is 8.314 J middot mol^-1-K^-1 The equilibrium expression for K_c for the reaction 4 NH_3(g) + 3 0_2(g) 4 NO(g) + 6 H_20(g) is: The reaction between sulfur dioxide and oxygen to form SO_3(g) is represented by the chemical reaction: 2 SO_2(g) + O_2(g) 2 SO_3(g) Equilibrium concentrations of the three gases were measured at a temperature of 1500 K and found to be 0.424 mol middot L^-1 for SO_2, 0.212 mol-L^-1 for O_2, and 0.076 mol-L^-1 for SO_3. The value of K_C for the reaction at a temperature of 1500 K is For the reaction N2(g) + 3H_2 (g) 2 NH_3(g) at a temperature of 773 K, the value of Kc is 2.86 middot 1O^-1. The corresponding value of K_p is The correct and meaningful expression for the equilibrium constant, K_c, in the reaction C(s) + CO_2(g) 2 CO(g)Explanation / Answer
Answer – 1) We are given the reaction
4NH3(g) + 3 O2(g) <-----> 4 NO(g) + 6 H2O(g)
We know the equilibrium constant expression, Kc and in Kc expression there is only gases and aqueous phases consider.
Kc = [H2O(g)]6[NO(g)]4 / [NH3(g)]4[O2(g)]3
2) We are given reaction –
2SO2(g) + O2(g) <---> 2 SO3(g)
T = 1500 K , at equilibrium [SO2(g)] = 0.424 M , [O2(g)] = 0.212 M ,
[SO3(g)] = 0.076 M
We know the Kc expression for this reaction –
Kc = [SO3(g)]2 / [SO2(g)] [O2(g)]
= (0.076)2 / (0.424)2 * (0.212)
= 0.152
3) We are given reaction
N2(g) + 3H2(g) <---> 2 NH3(g) , Kc = 0.286 , T = 773 K ,
We know formula
Kp = Kc (RT)n
n = sum of the moles of product – sum of the moles of reactant
= 2 – 4
= -2
Kp = 0.286 * (0.0821 *773)-2
= 7.10*10-5
4) We are given reaction
C(s) + CO2(g) <---> 2 CO(g)
We know the equilibrium constant expression, Kc and in Kc expression there is only gases and aqueous phases consider.
Kc = [CO(g)]2 / [CO2(g)]
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