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FAQs on Advanced Level MCQs Question Bank - Chemical Equilibrium - JEE
| 1. What is chemical equilibrium and how is it achieved? |  |
Ans. Chemical equilibrium is a state in a chemical reaction where the concentrations of reactants and products remain constant over time. It is achieved when the forward and backward reactions occur at the same rate, resulting in no net change in the concentrations of reactants and products. This dynamic balance is typically reached when the system is closed and isolated, allowing the reaction to reach a state of equilibrium.
| 2. How does temperature affect chemical equilibrium? | |
Ans. Temperature has a significant effect on chemical equilibrium. According to Le Chatelier's principle, an increase in temperature favors the endothermic reaction, while a decrease in temperature favors the exothermic reaction. This means that if the forward reaction is endothermic, increasing the temperature will shift the equilibrium towards the products, while decreasing the temperature will shift it towards the reactants. Similarly, if the forward reaction is exothermic, increasing the temperature will shift the equilibrium towards the reactants, while decreasing the temperature will shift it towards the products.
| 3. Can the concentration of reactants and products at equilibrium be altered? | |
Ans. The concentrations of reactants and products at equilibrium are determined by the equilibrium constant (K). However, it is possible to alter the concentrations by changing the conditions of the system. By increasing or decreasing the concentrations of reactants or products, the equilibrium can be shifted towards the side with higher concentration. This is known as the principle of Le Chatelier. However, it is important to note that the value of the equilibrium constant remains constant, regardless of the concentrations.
| 4. How does pressure affect chemical equilibrium? | |
Ans. Pressure has a significant effect on chemical equilibrium, particularly for reactions involving gases. According to Le Chatelier's principle, an increase in pressure will shift the equilibrium towards the side with fewer moles of gas, while a decrease in pressure will shift it towards the side with more moles of gas. This is because an increase in pressure favors the reaction that decreases the total number of gas moles, while a decrease in pressure favors the reaction that increases the total number of gas moles.
| 5. What factors can disrupt chemical equilibrium? | |
Ans. Chemical equilibrium can be disrupted by several factors, including changes in temperature, pressure, and concentration. Additionally, the addition or removal of a catalyst can also disrupt the equilibrium. Any change that causes the equilibrium to shift towards either the reactants or the products will disrupt the equilibrium. It is important to note that the system will eventually adjust to the new conditions and establish a new equilibrium.
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