Chemistry College

Please help
Apply your knowledge and understanding of equilibrium constant in solving the following problems:

The equilibrium constant Kc for the reaction below is 170 at 500 K.

Determine whether the reaction mixture is at equilibrium when the concentrations of the components at this temperature are as follows:
[N2]=1.50
[H2]=1.00
[NH3]=8.00

If it is not at equilibrium, state and explain in which direction the reaction will proceed.Multi Line Text.
2()+32() ⇄ 23()

Answers

Answer 1

Answer:

The reaction will proceed to the right to attain the equilibrium.

Explanation:

Step 1: Write the balanced equation

2 N₂(g) + 3 H₂(g) = 2 NH₃(g)

Step 2: Calculate the reaction quotient

The reaction quotient (Qc) is calculated in the same way as the equilibrium constant (Kc) but it uses the concentrations at any time.

Qc = [NH₃]² / [N₂]² × [H₂]³

Qc = 8.00² / 1.50² × 1.00³ = 28.4

Since Qc ≠ Kc, the reaction is not at equilibrium.

Since Qc < Kc, the reaction will proceed to the right to attain the equilibrium.

Related Questions

How long will it take a 500-W heater to raise the temperature of 400 g of water from 15.0 °C to 98.0
°C?

Answers

Explanation:

E=(98-15)×400×4.2

E=139440J

t=E/P

E=139440/500=278.88s

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