Question

The equilibrium constant for the reaction Ni (s) + 4 CO (g)imageNi(CO)4 (g) is 62,599.3 at a certain temperature. What is the value of the equilibrium constant for the reaction below, at that same temperature? ½ Ni(CO)4 (g)image½ Ni(s) + 2 CO (g)

Answer 1

The equilibrium constant for the reaction ½ Ni(CO)4 (g) ⇆ ½ Ni(s) + 2 CO (g) is 0.00400

Step-by-step explanation:

Step 1: Data given

Ni (s) + 4 CO (g) ⇆ Ni(CO)4 (g) Kc = 62599.3

Step 2: The balanced equation

½ Ni(CO)4 (g) ⇆ ½ Ni(s) + 2 CO (g)

Step 3: Calculate Kc for the reverse reaction

Ni(CO)4 (g) ⇆ Ni (s) + 4 CO (g)

Kc' = 1/Kc

Kc' = 1/ 62599.3

Kc' = 1.60*10^-5

Step 4: Calculate Kc for half of the reaction

½ Ni(CO)4 (g) ⇆ ½ Ni(s) + 2 CO (g)

Kc" = √(Kc')

Kc" = √(1.60*10^-5)

Kc" = 0.00400

The equilibrium constant for the reaction ½ Ni(CO)4 (g) ⇆ ½ Ni(s) + 2 CO (g) is 0.00400

Answer 2

K = 4.00x10⁻³

Step-by-step explanation:

Ni(s) + 4CO(g) → Ni(CO)₄(g)

Where equilibrium constant, K, is defined as:

K₁ = [Ni(CO)₄] / [CO] = 62599.3

The inverse reaction, has a K of:

Ni(CO)₄(g) → Ni(s) + 4CO(g)

K₂ = [CO] / [Ni(CO)₄]

K₂ = 1/K₁ = 1 / 62599.3 = 1.59746x10⁻⁵

Now, if reaction with the reaction decreases its coefficients in the half, K is:

¹/₂ Ni(CO)₄(g) → ¹/₂Ni(s) + 2 CO(g)

K₃ = √[CO] / √[Ni(CO)₄] = √K₂ = √1.59746x10⁻⁵ = 4.00x10⁻³