Consider the equilibrium reaction: 3cio-(aq) ↔ cio3-(aq) + 2ci-(aq) the equilibrium constant kc = 3.2 x 103. the following concentrations are present: [cl-] = 0.50 mol/l; [clo3-] = 0.32 mol/l; [clo-] = 0.24 mol/l. is the mixture at equilibrium and, if not, in which direction will reaction proceed?

Forward direction

Explanation:

The reaction quotient of an equilibrium reaction measures relative amounts of the products and the reactants present during the course of the reaction at  particular point in the time.

Q < Kc , reaction will proceed in forward direction.

Q > Kc , reaction will proceed in backward direction.

Q = Kc , reaction at equilibrium.

It is the ratio of the concentration of the products and the reactants each raised to their stoichiometric coefficients. The concentration of the liquid and the gaseous species does not change and thus is not written in the expression.

Thus, for the reaction:

The expression is:

Given,

[Cl⁻] = 0.50 mol/L; [ClO₃⁻] = 0.32 mol/L; [ClO⁻] = 0.24 mol/L

So,

Q = 5.7870

Since, Q < Kc ()

The reaction will go in forward direction.

a. a clone will be physically identical to the original, but won’t be genetically identical

have a good day!

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm