Question

Which of the following equilibrium systems most favors the products? a) CI2(g) + 2NO2(g) 2NO2CI(g); Keq = 1.8 b) N2(g) + 3H2(g) 2NH3(g); Keq = 345 c) 2HCI2(g) H2(g) + CI2(g); Keq = 2.0 × 10-7 d) CI2(g) + 2NO(g) 2NOCI(g); Keq = 3.7 × 108

Answer 1

CI2(g) + 2NO(g) 2NOCI(g); Keq = 3.7 × 10^8

Answer 2

Answer: The correct answer is Option d.

Step-by-step explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
`K_(eq)`

For a general chemical reaction:

`aA+bB\rightarrow cC+dD`

The expression for
`K_(eq)` is written as:

`K_(eq)=([C]^c[D]^d)/([A]^a[B]^b)`

There are 3 conditions:

• When
  `K_(eq)>1`; the reaction is product favored.
• When
  `K_(eq)<1`; the reaction is reactant favored.
• When
  `K_(eq)=1`; the reaction is in equilibrium.

From the above expression, the equilibrium constant is directly dependent on product concentration. Thus, more is the concentration of product, more will be the equilibrium constant.

The highest values of
`K_(eq)` will favor the product more.

Hence, the correct answer is Option d.