A mixture of CO(g) and H2(g) is pumped into a previously evacuated 2.0 L reaction vessel. The total pressure of the reaction system is 1.2 atm at equilibrium. What will be the total equilibrium pressure of the system if the volume of the reaction vessel is reduced to 1.0 L at constant temperature

The total equilibrium pressure of the system if the volume of the reaction vessel is reduced to 1.0 L at constant temperature = 2.4 atm

Explanation:

                   Total pressure of the system (P₁) = 1.2 atm at equilibrium

                   Volume (V₁) = 2.0 lit

                   If the volume of the reaction vessel is reduced to (V₂)= 1.0 lit

                   Pressure (P₂) ?

At constant temperature using Boyle's law

                        p₁v₁ = p₂v₂

Total pressure at equilibrium is equal to 2.4 atm.

since electrons are negative the answer is neagtaive

the dissociation of nickel hydroxide is follows:

the concentration of hydroxide ion is

the equilibrium constant value of nickel hydroxide is = 6.1 * 10^-^1^6 and thus equilibrium equation can be written as:

thus, concentration of ni is 0.23 * 10^-^4 mol /l