Chemistry - Chemical Equilibrium Question with Solution | TestHub
Match Column I with Column II
Column I | Column II |
|---|---|
P) N2O4(g) ⇌ 2NO2(g) | i) Kp > Kc at 400 K |
Q) H2(g) + CO2(g) ⇌ H2O(g) + CO(g) | ii) Kp < Kc at 400 K |
R) 2SO2(g) + O2(g) ⇌ 2SO3(g) | iii) P is increased, reaction moves to right side |
S) CaCO3(s) ⇌ CaO(s) + CO2(g) | iv) Inert gas added at constant volume, equilibrium will not be affected |
| v) Inert gas added at constant pressure, equilibrium will shift right |
Options:
Answer:
Solution:
The relationship between and is given by the equation . At 400 K, .
Therefore:
- If , then .
- If , then .
For P: , which means (i). An inert gas at constant volume causes no change (iv). An inert gas at constant pressure shifts the equilibrium toward more moles, i.e., to the right (v). A pressure increase shifts the equilibrium to the left, so (iii) is incorrect.
For Q: , which means . In this case, there is no effect from pressure or inert gas, so only (iv) applies.
For R: , which means (ii). A pressure increase shifts the equilibrium to the right (iii). An inert gas at constant volume causes no change (iv). An inert gas at constant pressure shifts the equilibrium to the left, so (v) is incorrect.
For S: Only CO₂ is gaseous, so . This implies (i). An inert gas at constant volume causes no change (iv). An inert gas at constant pressure shifts the equilibrium to the right (v). A pressure increase shifts the equilibrium to the left, so (iii) is incorrect.
The correct mapping is option (d).
