calculations involving equilibrium constants

Question 1

write the expression for the equilibrium constant kc for the reaction:
aA+bB↔cC+dD.

Answer 1

kc = [C]c[D]d/[A]a[B]b
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Question 2

given the reaction N2(g) + 3H2(g) ↔️ 2NH3(g), how would you calculate the equilibrium constant kc?

Answer 2

kc = [NH3]2/[N2][H2]3

Question 3

if kc for a reaction is much greater than 1, what does this indicate about the position of equilibrium?

Answer 3

if kc is much greater than 1, the position of equilibrium lies to the right, indicating a higher concentration of products compared to reactants.

Question 4

how do you convert the equilibrium constant from concentration (kc) to pressure (kp) for gases?

Answer 4

kp = kc(rt)🔼n, where 🔼n is the difference in moles of gaseous products and reactants, r is the gas constant, and t is the temperature in kelvin.