For the reaction R → P, the concentration of a reactant changes from 0.03 M to 0.02 M in 25 minutes.
The average rate of reaction in M sec-1 is-

1. 6.67×10-5 M s-1
2. 5.67×10-5 M s-1
3. 6.67×10-6 M s-1
4. 5.67×10-6 M s-1
Subtopic:  Definition, Rate Constant, Rate Law |
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In a reaction, 2A → Products, the concentration of A decreases from 0.5 mol L−1 to 0.4 mol L−1 in 10 minutes.
The rate during this interval is-

1. 5×10-3M min-1
2. 8×10-3M min-1
3. 9×10-3M min-1
4. 3×10-3M min-1
Subtopic:  Definition, Rate Constant, Rate Law |
66%
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For a reaction, A + B → Product; the rate law is given by, r=k[A]1/2[B]2. The order of the reaction is:
 1 -1.5 2 1.5 3 0.5 4 2.5
Subtopic:  Order, Molecularity and Mechanism |
77%
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The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times, then the rate of formation of Y will -

1. Decreases by 3 times
2. Increase by 3 times
3. Decreases by 9 times
4. Increase by 9 times

Subtopic:  Order, Molecularity and Mechanism |
74%
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A first order reaction has a rate constant 1.15 x 10−3 s−1. The time required to convert 5g of this reactant into 3g is-

1. 424 s
2. 444 s
3. 464 s
4. 484 s

Subtopic:  First Order Reaction Kinetics |
61%
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Time required to decompose SO2Cl2 to half of its initial amount is 60 minutes. If the decomposition is a first order reaction, the rate constant of the reaction in sec-1 is-

1. 1.9×10-4 s-1
2. 1.7×10-4 s-1
3. 2.2×10-4 s-1
4. 1.6×10-4 s-1
Subtopic:  First Order Reaction Kinetics |
66%
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Rate constant (k) and temperature (T) are related  as :

1. $$k \,\, = A\, \, e^{\frac{-E_{a}}{RT}}$$
2. $$k \,\, = A\, \, e^{\frac{RT}{-E_{a}}}$$
3. $$k \,\, = A\, \, e^{\frac{E_{a}}{RT}}$$
4. None of the above
Subtopic:  Arrhenius Equation |
92%
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The rate of the chemical reaction doubles for an increase of 10 K in absolute temperature from 298 K. The value of Ea is-

1. 49.5 kJ mol-1
2. 52.9 kJ mol-1
3. 55.5 kJ mol-1
4. 57.9 kJ mol-1
Subtopic:  Arrhenius Equation |
62%
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