Q. No.Given that K is the rate constant for some order of any reaction at temperature T. Then the value of \(\lim\limits_{T \to \infty} log~k\) = (where A is the Arrhenius constant):
1. \(\frac{\text A}{2.303}\)
2. \(\text A\)
3. \(2.303~\text A\)
4. \(log~\text A\)
For the elementary reaction M N, the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M will be:
1. 4
2. 3
3. 2
4. 1
The rate constant value for a zero-order reaction is 2 x10-2 mol L-1 sec-1. If the concentration of the reactant after 25 sec is 0.5 M, then the initial concentration of reactant is:
1. 0.5 M
2. 1.25 M
3. 12.5M
4. 1.0 M
The rate constant for a second order reaction is 8x10-5 M-1 min-1 . How long will it take a 1M solution to be reduced to 0.5M?
1. 8.665 x 103 minute
2. 8 x 10-5 minute
3. 1.25 x 104 minute
4. 4x10-5 minute
The activation energy for a reaction is 9.0 kcal/mol. The increase in the rate constant when its temperature is increased from 298K to 308K is:
1. 10%
2. 100%
3. 50%
4. 63%
For a certain reaction of order \('n'\) the time for half change \(t_{1/2}\) is given by; 
\(=,t_{1/2}=\dfrac{2-\sqrt2}{K}\times C^{1/2}_0,\) where \(K\) is rate constant and \(C_0\) is initial concentration. The value of \(n\) is:
1. 1
2. 2
3. 0
4. 0.5
In the following first order competing reactions:
A + Reagent Product
B + Reagent Product
The ratio of K1/K2 if only 50% of B will have been reacted when 94% of A has been reacted in same time is:
1. 4.06
2. 0.246
3. 2.06
4. 0.06
For a reversible reaction A B, Ist order in both the directions, the rate of reaction is given by:
1. K1[A]
2. -K2B
3. K1[A] + K2[B]
4. K1[A] - K2[B]
The time for half-life of a first order reaction is 1 hr. What is the time taken for 87.5% completion of the reaction?
1. 1 hour
2. 2 hour
3. 3 hour
4. 4 hour
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