The rate constant k1 and k2 for two different reactions are 1016. e-2000/T and 1015.e-1000/T respectively. The temperature at which k1 = k2
1000 K
2000/2.303 K
2000 K
2000 K
D.
2000 K
The Arrhenius equation is represented as;
k = Ae-Ea/RT
In the given equations first, take log and then compare them.
If 60% of a first order reaction was completed in 60 min, 50% of the same reaction would be completed in approximately:
50 min
45 min
60 min
60 min
B.
45 min
The bromination of acetone cytosine and guanine solution is represented by this equation.
CH3COCH3 (aq) + Br2 (aq) →CH3COCH2Br (aq) + H+ (aq) + Br- (aq)
These kinetic data were obtained for given reaction concentrations.
|
Initial Concentrations, M
|
||
| [CH3COOH] | [Br2] | [H+] |
| 0.30 | 0.05 | 0.05 |
| 0.30 | 0.10 | 0.05 |
| 0.30 | 0.10 | 0.10 |
| 0.40 | 0.05 | 0.20 |
Rate = k[CH3COCH3][H+]
Rate = k[CH=COCH3][Br2]
Rate = k [CH3COCH3][Br2][H+]
Rate = k [CH3COCH3][Br2][H+]
A.
Rate = k[CH3COCH3][H+]
By comparing the rate and concentration, the order of the reaction can be calculated.
Let the rate of the reaction wrt [CH3COCH3], [Br2] and [H+] are x,y and z respectively. Thus, 
The reaction of hydrogen and iodine monochloride is given as:
H2 (g) + 2ICl (g) → 2 HCl (g) + I2 (g)
This reaction is of first order with respect to H2 (g) and ICI (g), following mechanisms were proposed:
Mechanism A:
H2 (g) + 2 ICl (g) → 2 HCl (g) + I2 (g)
Mechanism B:
H2 (g) + ICl (g) →HCl (g) + HI (g) ;slow
HI (g) + ICl (g) → HCl (g) + I2 (g); fast
Which of the above mechanism (s) can be consistent with the given information about the reaction?
B only
A and B both
Neither A nor B
Neither A nor B
B.
A and B both
The rate of reaction always depends on slow reaction.
H2 (g) + ICl (g) →HCl (g) + HI (g) is a first order reaction respect to H2 and I2 can measure with the help of both mechanism A and B.
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