For the reaction, 2NH₃ ⟶ N₂ + 3H₂, if \(\frac { -d[NH_{ 3 }] }{ dt } \) = k₁[NH₃], \(\frac { d[N_{ 2 }] }{ dt } =k_{ 2 }[NH_{ 3 }],\frac { d[{ H }_{ 2 }] }{ dt } \)= k₃[NH₃] then the relation between k₁, k₂ and k₃ is _________.

For a reaction Rate = k[acetone]^3/2 then unit of rate constant and rate of reaction respectively is _______.

In a reversible reaction, the enthalpy change and the activation energy in the forward direction are respectively −x kJ mol^-1 and y kJ mol^-1. Therefore, the energy of activation in the backward direction is _______.

For the reaction, 2N₂O₅ ⟶4 NO₂+O₂, select the correct statement.

The depletion of ozone involves the following steps:
Step 1: O₂ +O \(\overset { { k }_{ 1 } }{ \underset { { k }_{ 2 } }{ \rightleftharpoons } } \) O₃ (fast)
Step 2: O₃ +O \(\overset { k }{ \longrightarrow } \) 2O₂ (slow)
The predicted order of the reaction will be ______.

Describe the graphical representation of first order reaction.

Explain the effect of catalyst on reaction rate with an example.

The decomposition reaction of ammonia gas on platinum surface has a rate constant R = 2.5 x 10^-4mol L^-1. What is the order of the reaction.

The reaction A + 2B ⟶ C obeys the rate equation. Rate = \(K{ \left[ A \right] }^{ \frac { 1 }{ 2 } }{ \left[ B \right] }^{ \frac { 3 }{ 2 } }\) What is the order of the reaction?

The rate of the reaction X + 2y→ product is 4 x 10^-3 mol L^-1S^-1, if [X] = [Y] = 0.2M and rate constant at 400K is 2 x 10^-2s^-1, What is the overall order of the reaction.

For a reaction x + y + z\(\longrightarrow \) products the rate law is given by rate =k[x]^3/2[y]^1/2. What is the overall order of the reaction and what is the order of the reaction with respect to z.

Explain briefly the collision theory of bimolecular reactions.

A first order reaction is found to have a rate A constant k = 7.39 x 10^-5 S^-1. Find the half life of this reaction.

What is the effect of temperature on the rate constant of a reaction? How can this temperature effect on rate constant be represented quantitatively?

A first order reaction takes 8 hours for 90% completion. Calculate the time required for 80% completion. (log 5 = 0.6989 ; log10 = 1)

A zero order reaction is 20% complete in 20 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?

The activation energy of a reaction is 22.5 k Cal mol^-1 and the value of rate constant at 40°C is 1.8 x 10^-5s^-1. Calculate the frequency factor, A.

A first order reaction laws on rate constant 1.15 x 10^-3 S^-1. How long will 5 g of this reactant take to reduce to 3g?

The decomposition of NH₃ on platinum surface is zero reaction. What are the rate of production of N₂ and H₂ it K = 2.5 x 10^-4mol L^-1 S^-1?