NEET > Chemistry Class 11 > Short Tricks: Kp & Kc problems
Short Tricks: Kp & Kc problems Video Lecture - Chemistry Class 11 - NEET
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FAQs on Short Tricks: Kp & Kc problems Video Lecture - Chemistry Class 11 - NEET
| 1. What is the difference between Kp and Kc in chemical equilibrium? |  |
Ans. Kp and Kc are both equilibrium constants, but they are used to represent equilibrium concentrations in different ways. Kp represents the equilibrium constant in terms of partial pressures, while Kc represents the equilibrium constant in terms of molar concentrations. So, Kp is used when the reaction involves gases, and Kc is used when the reaction involves aqueous solutions or solids.
| 2. How do you calculate Kp from Kc? | |
Ans. To calculate Kp from Kc, you need to use the ideal gas law. The equation is Kp = Kc(RT)^(Δn), where R is the ideal gas constant, T is the temperature in Kelvin, and Δn is the change in the number of moles of gas between the products and reactants. By substituting these values into the equation, you can calculate Kp.
| 3. How can you determine the equilibrium constant Kp or Kc experimentally? | |
Ans. To determine the equilibrium constant experimentally, you need to measure the concentrations of reactants and products at equilibrium and use them to calculate the value of Kc. For Kp, you need to measure the partial pressures of gases at equilibrium. This can be done using various techniques such as spectroscopy, chromatography, or by analyzing the equilibrium position of a reaction at different concentrations or pressures.
| 4. Can the equilibrium constant Kp or Kc change with temperature? | |
Ans. Yes, the equilibrium constant Kp or Kc can change with temperature. According to Le Chatelier's principle, if the temperature is increased, the equilibrium will shift in the endothermic direction to absorb the excess heat, which can result in a change in the equilibrium constant. Similarly, if the temperature is decreased, the equilibrium will shift in the exothermic direction, also leading to a change in the equilibrium constant.
| 5. What does it mean if the equilibrium constant Kp or Kc is large or small? | |
Ans. If the equilibrium constant Kp or Kc is large, it means that the products are favored at equilibrium, and the reaction proceeds almost to completion. On the other hand, if the equilibrium constant is small, it means that the reactants are favored at equilibrium, and the reaction does not proceed significantly to the products. The magnitude of the equilibrium constant gives information about the relative concentrations of reactants and products at equilibrium.
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