Previous year questions with solutions · 2000 – 2026
| Year | Questions | Papers | Avg / paper | Weightage |
|---|---|---|---|---|
| 2026 | 4 | 2 | 2 | 4.44% ▼ 33.3% vs last year |
| 2025 | 3 | 1 | 3 | 6.67% ▲ 11.1% vs last year |
| 2024 | 6 | 2 | 3 | 6.00% ▲ 53% vs last year |
| 2023 | 2 | 1 | 2 | 3.92% ▼ 20.8% vs last year |
| 2022 | 5 | 2 | 2.5 | 4.95% ▲ 147.5% vs last year |
| 2021 | 1 | 1 | 1 | 2.00% ▼ 55% vs last year |
| 2020 | 2 | 1 | 2 | 4.44% ▼ 33.3% vs last year |
| 2019 | 3 | 1 | 3 | 6.67% same as last year |
| 2018 | 3 | 1 | 3 | 6.67% same as last year |
| 2017 | 3 | 1 | 3 | 6.67% ▲ 20% vs last year |
| 2016 | 5 | 2 | 2.5 | 5.56% same as last year |
| 2015 | 5 | 2 | 2.5 | 5.56% ▼ 37.5% vs last year |
| 2014 | 4 | 1 | 4 | 8.89% ▲ 31.9% vs last year |
| 2013 | 6 | 2 | 3 | 6.74% ▲ 7.9% vs last year |
| 2012 | 5 | 2 | 2.5 | 6.25% ▲ 1.3% vs last year |
| 2011 | 5 | 2 | 2.5 | 6.17% ▼ 1.2% vs last year |
| 2010 | 5 | 2 | 2.5 | 6.25% ▼ 20.3% vs last year |
| 2009 | 4 | 1 | 4 | 7.84% ▼ 33.3% vs last year |
| 2008 | 6 | 1 | 6 | 11.76% ▲ 47.1% vs last year |
| 2007 | 4 | 1 | 4 | 8.00% ▲ 33.3% vs last year |
| 2006 | 3 | 1 | 3 | 6.00% same as last year |
| 2005 | 3 | 1 | 3 | 6.00% ▲ 44% vs last year |
| 2004 | 2 | 1 | 2 | 4.17% ▼ 31.9% vs last year |
| 2003 | 3 | 1 | 3 | 6.12% ▼ 23.5% vs last year |
| 2002 | 4 | 1 | 4 | 8.00% ▲ 2% vs last year |
| 2001 | 4 | 1 | 4 | 7.84% same as last year |
| 2000 | 4 | 1 | 4 | 7.84% |
⚠ 1 of these questions are out of the current syllabus (marked on the question).
In which of the following equilibria, Kp and Kc are NOT equal?
At a given temperature and pressure, the equilibrium constant values for the equilibria are given below: 3A2 + B2 2A3B, K1 A3B 32A2 + 12B2, K2 The relation between K1 and K2 is :
The equilibrium constants of the following are N2 + 3H2 2NH3; K1 N2 + O2 2NO; K2 H2 + 12O2 H2O; K3 The equilibrium constant (K) of the reaction : 2NH3 + 52O2 2NO + 3H2O will be
If the equilibrium constant for N2(g) + O2(g) 2NO(g) is K, the equilibrium constant for 12 N2(g) + 12 O2(g) NO(g) will be
For a given exothermic reaction, Kp and K'p are the equilibrium constants at temperatures T1 and T2, respectively. Assuming that heat of reaction is constant in temperature range between T1 and T2, it is readily observed that
Given that the equilibrium constant for the reaction, 2SO2(g) + O2(g) 2SO3(g) has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature ? SO3(g) SO2(g) + 12O2(g)
For the reaction, N2(g) + O2(g) 2NO(g), the equilibrium constant is K1. The equilibrium constant is K2 for the reaction, 2NO(g) + O2(g) 2NO2(g) What is K for the reaction, NO2(g) 12N2(g) + O2(g)
The value of equilibrium constant of the reaction HI(g) 12H2(g) + 12I2(g) is 8.0. The equilibrium constant of the reaction H2(g) + I2(g) 2HI(g) will be
The equilibrium constants of the following are N2 + 3H2 2NH3; K1 N2 + O2 2NO; K2 H2 + 12O2 H2O; K3 The equilibrium constant (K) of the reaction: 2NH3 + 52O2 2NO + 3H2O will be
For the reaction : CH4(g) + 2O2(g) CO2(g) + 2H2O(l), Hr = -890.3 kJ mol-1. Which of the following statements is not true?
Equilibrium constants K1 and K2 for the following equilibria: NO(g) + 12O2(g) K1 NO2(g) and 2NO2(g) K2 2NO(g) + O2(g) are related as
The equilibrium constants of the following are N2 + 3H2 2NH3; K1 N2 + O2 2NO; K2 H2 + 12O2 H2O; K3 The equilibrium constant (K) of the reaction : 2NH3 + 52O2 2NO + 3H2O will be
Reaction BaO2(s) BaO(s) + O2(g); H = +ve. In equilibrium condition, pressure of O2 depends on
For any reversible reaction, if we increase concentration of the reactants, then effect on equilibrium constant
Equilibrium constant Kp for following reaction MgCO3(s) MgO(s) + CO2(g)