Question

Consider the reaction H2(g) + I2(g) <-> HI(g) with an equilibrium constant of 46.3 and a reaction quotient of 525. Which direction will the system shift to?

The equilibrium will shift to the left to favor the reactants.

The equilibrium will shift to the right to favor the products.

The equilibrium will not shift in any direction.

The equilibrium will shift to the forward reaction.

Answer 1

A

Step-by-step explanation:

A

Answer 2

Answer : The correct option is, The equilibrium will shift to the left to favor the reactants.

Explanation :

Reaction quotient (Q) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.

The given balanced chemical reaction is,

`H_2(g)+I_2(g)\rightleftharpoons 2HI(g)`

The expression for reaction quotient will be :

`Q=([HI]^2)/([H_2][I_2])`

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.

The given reaction quotient value is,
`Q=525`

The given equilibrium constant value is,
`K_c=46.3`

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

There are 3 conditions:

When
`Q>K_c` that means product > reactant. So, the reaction is reactant favored.

When
`Q<K_c` that means reactant > product. So, the reaction is product favored.

When
`Q=K_c` that means product = reactant. So, the reaction is in equilibrium.

From the above we conclude that, the
`Q>K_c` that means product > reactant. So, the reaction is reactant favored that means reaction must shift to the reactant (left) to be in equilibrium.

Hence, the correct option is, The equilibrium will shift to the left to favor the reactants.