Question

Consider the reaction: " id="TexFormula1" title="NiO(s)+CO(g) \rightleftharpoons Ni(s)+CO_2(g)" alt="NiO(s)+CO(g) \rightleftharpoons Ni(s)+CO_2(g)" align="absmiddle" class="latex-formula">; Kc=4.0×10³ at 1500 K.
If a mixture of solid nickel(II) oxide and 0.18000 MM carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of CO₂?

Answer 1

Answer:

Molar concentration of CO₂ in equilibrium is 0.17996M

Explanation:

Based on the reaction:

NiO(s) + CO(g) ⇆ Ni(s) + CO₂(g)

kc is defined as:

kc = [CO₂] / [CO] = 4.0x10³ (1)

As initial concentration of CO is 0.18M, the concentrations in equilibrium are:

[CO] = 0.18000M - x

[CO₂] = x

Replacing in (1):

4.0x10³ = x / (0.18000-x)

720 - 4000x = x

720 = 4001x

x = 0.17996

Thus, concentrations in equilibrium are:

[CO] = 0.18000M - 0.17996 = 4.0x10⁻⁵

[CO₂] = x = 0.17996M

Thus, molar concentration of CO₂ in equilibrium is 0.17996M

I hope it helps!