Exams › JEE Main › Chemistry

Higher order (> 3) reactions are rare due to: (1) Low probability of simultaneous collision of all the reacting species (2) Increase in entropy and activation energy as more molecules are involved (3) Shifting of equilibrium towards reactants due to elastic collisions (4) Loss of active species on collision

1. Low probability of simultaneous collision of all the reacting species
2. Increase in entropy and activation energy as more molecules are involved
3. Shifting of equilibrium towards reactants due to elastic collisions
4. Loss of active species on collision

Correct answer: Low probability of simultaneous collision of all the reacting species

Solution

Higher order reactions are uncommon because the likelihood of multiple molecules colliding at the exact same time decreases significantly as the number of reactants increases, making such reactions less probable.

Related JEE Main Chemistry questions

• If a biochemical reaction is performed in the laboratory without an enzyme and its rate is found to be 10^{-6} times, then the activation energy for the reaction in the presence of the enzyme is:
• For the reaction A \rightarrow products, the half-life is 120 min when the initial concentration of A is 8.0 \times 10^{-2} M. If the starting concentration is changed to 4.0 \times 10^{-2} M, the half-life increases to 240 min. What is the reaction order?
• For a first-order process A \rightarrow B, if the rate constant is k and the initial concentration of A is 0.5 M, what is the half-life?
• For the gas-phase reaction A(g) + B(g) \rightarrow C(g), the rate law is rate = k C_A^2 C_B^4. Which change in the initial concentrations of A and B will make the reaction rate eight times larger?
• For the elementary gas-phase reaction A(g) + 2B(g) \rightarrow C(g) + D(g), an experiment starts with initial partial pressures p_A = 0.60 atm and p_B = 0.80 atm. If the partial pressure of C becomes 0.20 atm, then the reaction rate compared with the initial rate is
• From the experimental data below for the reaction A + B \rightarrow products, identify the rate law that fits the observations. Exp. 1: [A] = 0.012, [B] = 0.035, initial rate = 0.1 Exp. 2: [A] = 0.024, [B] = 0.070, initial rate = 0.8 Exp. 3: [A] = 0.024, [B] = 0.035, initial rate = 0.1 Exp. 4: [A] = 0.012, [B] = 0.070, initial rate = 0.8

⚔️ Practice JEE Main Chemistry free + battle 1v1 →