Exams › NEET › Chemistry

The equilibrium constant for a reaction is \( K, \) and the reaction quotient is \( Q \). For a reaction mixture, the ratio \( \frac{K}{Q} \) is 0.33 This means that:

1. the reaction mixture will equilibrium to form more reactant species
2. the reaction mixture will equilibrium to form more product species
3. the equilibrium ratio of reactant to product concentrations will be 3
4. the equilibrium ratio of reactant to product concentrations will be 0.33

Correct answer: the reaction mixture will equilibrium to form more product species

Solution

Since K/Q = 0.33, Q is greater than K. That means the mixture has too much reactant relative to product compared with equilibrium, so the reaction shifts forward to make more products until Q = K.

Related NEET Chemistry questions

• Which of the following will change the value of the equilibrium constant for the reaction? \( N_{2}(g)+O_{2}(g) \leftrightharpoons 2 N O(g) \)
• The state of equilibrium refers to:
• For the following equilibrium, \( N_{2} O_{4} \rightleftharpoons \) \( 2 N O_{2} \) in gaseous phase, \( N O_{2} \) is \( 50 \% \) of the total volume when equilibrium is set up. Hence, percent of dissociation of \( N_{2} O_{4} \) is:
• One mole of ethanol is treated with one mole of ethanoic acid at \( 25 . \) One-forth of the acid changes into ester at equilibrium. The equilibrium constant for the reaction will be:
• The following reaction occurs in the Blast Furnace where ion ore is reduced to iron metal: \( \boldsymbol{F e}_{2} \boldsymbol{O}_{3}(\boldsymbol{s})+\boldsymbol{3} \boldsymbol{C O}(\boldsymbol{g}) \rightleftharpoons \boldsymbol{2} \boldsymbol{F} \boldsymbol{e}(l)+ \) \( 3 C O(g) \) Using Le Chatelier's principle, predict which of the following will not disturb the equilibrium?
• Haber's process is a/an:

⚔️ Practice NEET Chemistry free + battle 1v1 →