1.For the reaction R → P, the concentration of a reactant changes from 0.03 M to 0.02 M is 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.
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2.In a reaction 2A → Products, the concentration of A decreases from 0.5 mol to 0.4 mol L–1 in 10 minutes. Calculate the rate during this interval.
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3.For a reaction, A + B → Product; the rate law is given by, r = k[ A]1/2 [B]2. What is the order of reaction?
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4.The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?
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5.A first order reaction has a rate constant 1.15 x 10–3 s–1. How long will 5 g of this reactant take to reduce to 3 g?
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6.Time required to decompose SO2 Cl2 to half its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.
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7.What will be the effect of temperature on rate constant?
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8.The rate of the chemical reaction doubles for an increase of 10 k in absolute temperature from 298 K. Calculate Ea.
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9.
The activation energy for the reaction 2HI (g) → H2 + I2(g) is 209.5 kJ mol–1 at 581 k. Calculate the fraction of molecules of reactants having energy equal to or greater than activation energy?
10.For the reaction A B, the rate of reaction becomes twenty seven times when the concentration of A is increased three times. What is the order of the reaction?
r= k[A]n =Kan When concentration is increased three time [ A] =3a therefore,
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