Chemical Kineti...

The order of the reaction whose rate and rate constant are the same is

Activation energy of a chemical reaction can be determined by plotting

2A B + C

For the above reaction - d[A]/dt = k[A]²
The half life of the reactant is

The rate of a reaction is r₁ at 35^oC. The rate of a reaction at 45^oC will be

Given log 25 = 1.4

For a reaction, the rate constants at 200k and 400k temperatures are 50 x 10^-3 and 125 x 10^-2, respectively. The activation energy of the reaction (in kcals) will be

P₂O₅ P₂O₃ + O₂
Given that: - d[P₂O₅]/dt = k₁[P₂O₅]
+ d[P₂O₃]/dt = k₂[P₂O₅]
+ d[ O₂]/dt = k₃[P₂O₅]
[Neglect the feasibility of the reaction]

The relation between k₁, k₂ and k₃ is

Consider : a = initial concentration
a-x = current concentration at a time t

A straight line is drawn taking 1/a-x on y-axis and time on x-axis with a slope equal to rate constant with an intercept 1/a on y-axis. What is the order of the reaction?

If the concentration is made x times for an n^th order reaction, then the change in rate will be

In a certain first order reaction after 10 minutes, the volume of the product formed is 90 litres and after completion of reaction, the product formed is 100 litres. The value of rate constant k (mole/lit.sec) is

The half-life periods of four reactions A, B, C and D are 25 sec, 1.5 minutes, 200 sec and 0.2 minutes, respectively. The fastest reaction is

What is the rate of a first order reaction whose half life is 10 seconds and initial concentration is 10 mole/lit?

C₁₂H₂₂O₁₁ + H₂ O C₆H₁₂O₆ + C₆H₁₂O₆

The order of the above reaction is

SO₂ + O₂ 2SO₃

If the rate of disappearance of sulphur dioxide is 0.01 moles/lit, the rate of appearance of sulphur trioxide will be

H₂ + I₂ 2HI
Given that - d[H₂]/dt = k₁[H₂][I₂]
- d[I₂]/dt = k₂[H₂][I₂]
+1/2 d[HI]/dt = k₃[H₂][I₂]

What is the relation between k_1,k₂ and k₃?