Chemical Kinetics

Which of the following statement is not true for radioactive decay?

1. Half life is 2 times of 1rate constant.
2. Decay constant increases with increase in temperature.
3. Decay constant does not depend upon temperature.
4. Amount of radioactive substance remained after three half lives is 18th of original amount.

Consider the given figure and choose the correct option : [figure]

1. Activation energy of both forward and backward reaction is E1 + E2 and reactant is more stable than product.
2. Activation energy of forward reaction is E1 + E2 and product is more stable than reactant.
3. Activation energy of backward reaction is E1 and product is more stable than reactant.
4. Activation energy of forward reaction is E1 + E2 and product is less stable than reactant.

Given below are two statements : Statement I : The rate law for the reaction A + B C is rate (r) = k[A]2[B]. When the concentration of both A and B is doubled, the reaction rate is increased "x" times. Statement II : [figure] The figure is showing "the variation in concentration against time plot" for a "y" order reaction. The value of x + y is .

Consider the following first order gas phase reaction at constant temperature A(g) 2B(g) + C(g) If the total pressure of the gases is found to be 200 torr after 23 sec. and 300 torr upon the complete decomposition of A after a very long time, then the rate constant of the given reaction is 10-2 s-1 (nearest integer) [Given : 10(2) = 0.301]

Consider the following reaction A + B C The time taken for A to become 1/4th of its initial concentration is twice the time taken to become 1/2 of the same. Also, when the change of concentration of B is plotted against time, the resulting graph gives a straight line with a negative slope and a positive intercept on the concentration axis. The overall order of the reaction is .

For a reaction A K1 B K2 C. If the rate of formation of B is set to be zero then the concentration of B is given by :

1. (K1 - K2)[A]
2. (K1 + K2)[A]
3. K1K2[A]
4. (K1/K2)[A]

Time required for 99.9\% completion of a first order reaction is times the time required for completion of 90\% reaction.(nearest integer)

Consider the two different first order reactions given below A + B C (Reaction 1) P Q (Reaction 2) The ratio of the half life of Reaction 1 : Reaction 2 is 5 : 2. If t1 and t2 represent the time taken to complete 2/3rd and 4/5th of Reaction 1 and Reaction 2, respectively, then the value of the ratio t1 : t2 is 10-1 (nearest integer). [Given : 10(3) = 0.477 and 10(5) = 0.699]

During kinetic study of reaction 2A + B C + D, the following results were obtained : [figure] Based on above data, overall order of the reaction is .

Consider the following single step reaction in gas phase at constant temperature. 2A(g) + B(g) C(g) The initial rate of the reaction is recorded as r1 when the reaction starts with 1.5 atm pressure of A and 0.7 atm pressure of B. After some time, the rate r2 is recorded when the pressure of C becomes 0.5 atm. The ratio r1 : r2 is 10-1. (Nearest integer)