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Chemical Kinetics

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Q.

A catalysts is used

Q.

The concentration of R in the reaction RP was measured as a function of time and the following data is obtained

[R](molar)

1.00

0.75

0.40

0.10

t (min)

0.00

0.05

0.12

0.18

The order of the reaction is

Q.

For a zero order reaction, the plot of concentration, vs time is linear with

Q.

A substance “A” decomposes in solution following the first order kinetics. Flask I contains 1 L of 1 M solution of A and flask II contains 100 mL of 0.6 M solution. After 8 hr, the concentration, of A in flask I becomes 0.25 M. What will be the time for concentrating of A in flask II to become 0.3 M?

Q. Thermal decomposition of azo – isopropane to hexane and nitrogen follows a first order kinetics. If Pi is the initial pressure of arz – isopropane and the pressure after time t sec is P, then the expression for rate constant 'k' can be given by: a) 1/t ln p/2pi b) 1/t ln pi/p c) 1/t ln pi/(2pi-p) d) 1/t ln p/(2pi-p)?

Let p i​be the initial pressure of azoisopropane and at time t, p atm of azoisopropane decomposes. (CH 3​) 2​CHNH=NHCH(CH 3​) 2​⟶N 2​+C 6​H 14​At time, t=0 P azoisopropane​=P i​P N 2​​=0 P C 6​H 14​​=0 At time, t P azoisopropane​=P i​−p P N 2​​=p P C 6​H 14​​=p (The pressure is in atm.) Total pressure, P t​=(P i​−p)+p+p p=P t​−P i​P azoisopropane​=2P i​−P t​k= t 2.303​log [A] [A] 0​​k− t 2.303​log 2P i​−P t​P i​​When time is 360 s, k= 360 2.303​log 2×35.0−54 35.0​k=2.17×10 −3 /s When time is 720 s, k= 720 2.303​log 2×35.0−63.0 35.0​k=2.24×10 −3 /s Average value of k =2.20×10 −3 /s