Define average rate and instantaneous rate.

Define rate law and rate constant.

Derive integrated rate law for a zero order reaction A\(\longrightarrow \) product.

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

The rate law for a reaction of A, B and C has been found to be rate = k[A]²[B][L]^3/2 How would the rate of reaction change when
(i) Concentration of [L] is quadrupled
(ii) Concentration of both [A] and [B] are doubled
(iii) Concentration of [A] is halved
(iv) Concentration of [A] is reduced to \(\left(\frac{1}{3}\right)\) and concentration of [L] is quadrupled.

For a reaction A + B ⟶ C, the rate of the reaction is denoted \(\frac { -dA }{ dt } \) or \(\frac { -dB }{ dt } \) or \(\frac { +dC }{ dt } \). State the significance of plus and minus sign.

Rate of chemical reaction is not uniform throughout. Justify you answer:

H_2(g) + Cl_2(g) \(\overset { hv }{ \longrightarrow } \) 2HCl(g). The reaction proceeds with a uniform rate throughout. What do you conclude? 

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?

How does the value of rate constant vary with reactant constant.

In a reaction, 2A \(\longrightarrow \) products, the concentration of A decreases from 0.5 mol L^-1 to 0.4 mol L^-1 in 10 minutes. Calculate the rate during this interval?

Consider the oxidation of nitric oxide to form NO₂
2NO_(g) + O_2(g) ➝2NO_2(g)
(a). Express the rate of the reaction in terms of changes in the concentration of NO,O₂ and NO₂.
(b). At a particular instant, when [O₂] is decreasing at 0.2 mol L⁻¹s⁻¹ at what rate is [NO₂] increasing at that instant?

What is the order with respect to each of the reactant and overall order of the following reactions?
a) 5Br^-_(aq)+BrO₃^-_(aq)+6H⁺_(aq) ➝3Br_2(l)+3H₂O_(l)
The experimental rate law is Rate = k [Br⁻][BrO₃⁻][H⁺]²
b) CH₃CHO_(g)\(\overset { \Delta }{ \longrightarrow } \) CH_4(g)+CO_(g) the experimental rate law is
Rate =K[CH₃CHO]^{\(\frac{3}{2}\)}

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.