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Chemistry MCQs for NEET — Practice Questions with Answers

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Collision theory is most satisfactory for __________ reaction.

A. First order B. second order C. Bimolecular D. Any

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Explanation

Bimolecular

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If $E_f$ and $E_r$ are the activation energies of the forward and reverse reactions and the reaction is known to be exothermic then

$ E_f \lt E_r $

$ E_f \gt E_r $

$ E_f \gt \gt \gt E_r $

$ E_f = E_r $

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Explanation

$ E_f \lt E_r $

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Which of the following does not affect the rate of reaction ?

A. size of the vessel B. physical state of reactants C. amount of the reactants D. OH of reaction

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Explanation

OH of reaction

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For an endothermic reaction, OH represents the enthalpy of reaction. The minimum value for the energy of activation will be ...

A. equal to OH B. zero C. more than OH D. less than OH

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Explanation

more than OH

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For an endothermic reaction $ A --> B . An activation energy of 15 Kcal mole^{-1} and the enthalpy change of reaction is 5 Kcal mole^{-1} . The activation energy for the reaction B --> A $ is

A. $ 10 Kcal mole^{-1} $ B. $ 20 Kcal mole^{-1 } $ C. $ 15 Kcal mole^ {-1} $ D. zero

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Explanation

10 Kcal $ mole^{-1} \triangle H = Ea - Ea^r \therefore +5 = 15 - Ea ^5 \therefore Ea^r = 10 $

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For an exothermic reaction an activation energy of $ 70 KJ mole^{-1} $ and the enthalpy change of reaction is $ 30 KJ mole^{-1} $ . The activation energy for the reverse reaction is ...

A. $ 70 KJ mole^{-1} $ B. $ 30 KJ mole^{-1} $ C. $ 40 KJ mole^{-1} $ D. $ 100 KJ mole^{-1} $

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Explanation

100 Kj $ mole ^ {-1} \triangle H = Ea - Ea^r -30 = 70 - Ea^r \therefore Ea^r = 100 $

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The rate constant of the reaction increases by ...

A. increasing the temperature B. increasing the concentration of reactants C. carrying out the reaction for longer period D. adding catalyst

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Explanation

increasing the temperature.

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Which of the following is the expression for Arrhenius equation ?

A. $ ln { k_2 \over k_1 } = { Ea \over R } \left( {1 \over T_1 } - { 1 \over T_2 } \right) $ B. $ ln k = lnA - { Ea / RT } $ C. $ k = A.e ^ { -Ea/ RT } $ D. All the above

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Explanation

All the above

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The Plot of log $ K vs {1 \over T } $ helps to calculate

A. Activation energy B. Rate constant C. Reaction order D. Activation energy and frequency factor

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Explanation

Activation energy and frequency factor.

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At 290 K velocity constant of a reaction was found to be $ 3.2 \times 10^ {-3} $ . At 300 K, it will be

A. $ 1.6 \times 10 ^ {-3} $ B. $ 6.4 \times 10 ^ {-3} $ C. $ 3.2 \times 10 ^ {-4} $ D. $ 3.2 \times 10 ^ {-2} $

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Explanation

$ 3.2 \times 10^{â€“4} 10k $ rise, the velocity constant becomes nearly double

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