Question

i need help on question 2For each of the reactions below, write the (i)equilibrium constant expression, (ii) find its value,and (iii) determine if it’s reactant-favored, product-favored, or neither.(a) N 2 (g) + 3 H 2 (g) -----> 2 NH 3 (g)[N 2 ]eq = 1.50 M [H 2 ]eq = 2.00 M[NH 3 ]eq = 0.01 M(b)HF(aq) -----> H + (aq) + F – (aq)[HF] eq = 0.55 M [H + ] eq = 0.001 M[F – ] eq = 0.001 M(c) Fe 3+ (aq) + SCN – (aq) -----> FeSCN 2+ (aq)[Fe 3+ ] eq = 0.55 M [SCN – ] eq = 0.001M[FeSCN 2+ ] eq = 0.001 M

Answer 1

Step-by-step explanation

Part A

Given:

a) N₂ (g) + 3H₂ (g) -----> 2NH₃ (g)

[N₂ ]eq = 1.50 M, [H₂ ]eq = 2.00 M, [NH 3 ]eq = 0.01 M

Solution:

i. The equilibrium constant expression for the reaction is

`Kc=([NH_3]^2)/([N_2][H_2]^3)`