Question

5. For a reaction A+B ------>products, rate = k[A][B]? then what will be the unit of k?
(A) mols L-3 min
(B) mol L - min!
(C) mol-?L? min
(D) mol-min​

Answer 1

Explanation:

General unit for rate constant =(

General unit for rate constant =( L

General unit for rate constant =( Lmol

General unit for rate constant =( Lmol

General unit for rate constant =( Lmol )

General unit for rate constant =( Lmol ) 1−n

General unit for rate constant =( Lmol ) 1−n s

General unit for rate constant =( Lmol ) 1−n s −1

General unit for rate constant =( Lmol ) 1−n s −1

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction)

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =(

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( L

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing,

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, (

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( L

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol )

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =(

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( L

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol )s

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol )s −1

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol )s −1

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol )s −1 1−n=1

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol )s −1 1−n=1⇒n=0

General unit for rate constant =( Lmol ) 1−n s −1 (where, n= order of reaction) Given, unit for rate constant =( Lmol )s −1 On comparing, ( Lmol ) 1−n s −1 =( Lmol )s −1 1−n=1⇒n=0Hence, the order of the reaction is zero.

Answer 2

Answer:

For a reaction, A+B→P

For a reaction, A+B→PR1=k[A][B]2 ---------(i)

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2R2R1=4B2B2

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2R2R1=4B2B2R2=4R1

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2R2R1=4B2B2R2=4R1The rate of reaction will be four times the initial rate.

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2R2R1=4B2B2R2=4R1The rate of reaction will be four times the initial rate.(ii) If A is present in large excess, then the rate of the reaction will be independent of A and will depend only on the concentration of B. The overall rate of the reaction will be 2.        

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2R2R1=4B2B2R2=4R1The rate of reaction will be four times the initial rate.(ii) If A is present in large excess, then the rate of the reaction will be independent of A and will depend only on the concentration of B. The overall rate of the reaction will be 2.        (b) K=0.693/30=0.0231

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2R2R1=4B2B2R2=4R1The rate of reaction will be four times the initial rate.(ii) If A is present in large excess, then the rate of the reaction will be independent of A and will depend only on the concentration of B. The overall rate of the reaction will be 2.        (b) K=0.693/30=0.0231The time required to complete 90% reaction,

For a reaction, A+B→PR1=k[A][B]2 ---------(i)If the concentration of B is doubled,R2=k[A][2B]2---------(ii)On dividing (i) and (ii)R2R1=k[A][2B]2k[A][B]2R2R1=4B2B2R2=4R1The rate of reaction will be four times the initial rate.(ii) If A is present in large excess, then the rate of the reaction will be independent of A and will depend only on the concentration of B. The overall rate of the reaction will be 2.        (b) K=0.693/30=0.0231The time required to complete 90% reaction,t=(2.303/.0231)×log(100/10)=100minutes