Practice free Equilibrium (Chemistry) NEET multiple-choice questions online with instant answers and detailed explanations. No login required.
What is the primary condition for equilibrium to be possible in a physical process?
Under '6.1.5 General Characteristics of Equilibria Involving Physical Processes', point (i) states: 'Equilibrium is possible only in a closed system at a given temperature.'
In the Haber process for ammonia synthesis, experiments demonstrated that the reaction could reach equilibrium starting from different initial conditions (e.g., with $ ext{H}_2$ and $ ext{N}_2$ or with just $ ext{NH}_3$). This illustrates that equilibrium:
The NCERT text states: 'Similarly, the reaction can reach the state of equilibrium even if we start with only C and D; that is, no A and B being present initially, as the equilibrium can be reached from either direction.'
An equilibrium mixture is defined as:
The NCERT text states: 'The mixture of reactants and products in the equilibrium state is called an equilibrium mixture.'
The extent to which reactions proceed to reach chemical equilibrium can be classified into three groups. Which group describes reactions where concentrations of reactants and products are comparable at equilibrium?
The NCERT text lists three groups: '(i) The reactions that proceed nearly to completion...', '(ii) The reactions in which only small amounts of products are formed...', and '(iii) The reactions in which the concentrations of the reactants and products are comparable, when the system is in equilibrium.'
What happens to the rates of forward and reverse reactions during the approach to chemical equilibrium?
The NCERT text (Fig. 6.2 and accompanying description) explains: 'With passage of time, there is accumulation of the products C and D and depletion of the reactants A and B (Fig. 6.2). This leads to a decrease in the rate of forward reaction and an increase in the rate of the reverse reaction. Eventually, the two reactions occur at the same rate and the system reaches a state of equilibrium.'
For a chemical reaction, if the value of the equilibrium constant ($K_c$) is $2.4 \times 10^{47}$, what can be inferred about the extent of the reaction?
According to the NCERT text, 'If $K_c > 10^3$, products predominate over reactants, i.e., if $K_c$ is very large, the reaction proceeds nearly to completion.' A value of $2.4 \times 10^{47}$ is significantly greater than $10^3$.
Which of the following statements regarding the equilibrium constant ($K_c$) is INCORRECT?
The NCERT text states: 'The numerical value of the equilibrium constant for a reaction indicates the extent of the reaction. But it is important to note that an equilibrium constant does not give any information about the rate at which the equilibrium is reached.' Therefore, a large $K_c$ indicates extensive product formation at equilibrium, not a slow rate.
If the equilibrium constant ($K_c$) for a reaction is $5.0 \times 10^{-5}$, which of the following describes the composition of the equilibrium mixture?
As per the NCERT text, 'If $K_c < 10^{-3}$, reactants predominate over products, i.e., if $K_c$ is very small, the reaction proceeds rarely.' A value of $5.0 \times 10^{-5}$ is smaller than $10^{-3}$.
For the reaction $H_2(g) + Br_2(g) \rightleftharpoons 2HBr(g)$ at 300 K, the equilibrium constant ($K_c$) is $5.4 \times 10^{18}$. What does this value suggest about the reaction?
The NCERT states, 'If $K_c > 10^3$, products predominate over reactants, i.e., if $K_c$ is very large, the reaction proceeds nearly to completion.' A $K_c$ value of $5.4 \times 10^{18}$ is very large, indicating a strong preference for product formation at equilibrium.
Consider a reaction with an equilibrium constant $K_c = 0.5$. Which of the following is true at equilibrium?
The NCERT implies that for intermediate $K_c$ values (between $10^{-3}$ and $10^3$), the concentrations of reactants and products are comparable. Since $K_c = 0.5$ falls within this range, both reactants and products will be present in comparable amounts.
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