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Plots showing the variation of the rate constant (k) with temperature (T) are given below. The plot that follows Arrhenius equation is [JEE 2010]
Option (A) is correct. K increases exponentially with a rise in T(K=Ae^{−Ea/RT}).
The Arrhenius plot is used to study the effect of temperature on reaction rates. The Arrhenius plot can also be used by extrapolating the line back to the yintercept to obtain the preexponential factor, A.
This factor is significant because A=pZ, where p is a steric factor and Z is the collision frequency. The preexponential, or frequency, the factor is related to the number of times molecules will hit in the orientation necessary to cause a reaction.
The rate constant for the reaction
2N_{2}O_{5} → 4NO_{2} + O_{2}
is 3.0 × 10^{–5} sec^{–1}. If the rate is 2.4 × 10^{–5} mol litre^{–1} sec^{–1}, then the concentration of N_{2}O_{5} (in mol litre^{–1})
is [JEE SCR 2000]
If I is the intensity of absorbed light and C is the concentration of AB for the photochemical process
AB + hv → AB*, the rate of formation of AB* is directly proportional to [JEE SCR 2001]
Consider the chemical reaction, N_{2}(g) + 3H_{2}(g) → 2NH_{3}(g). The rate of this reaction can be expressed in term of time derivative of concentration of N_{2}(g), H_{2}(g) or NH_{3}(g). Identify the correct relationship amongst the rate expressions. [JEE SCR 2002]
In a first order reaction the concentration of reactant decreases from 800 mol/dm^{3} to 50 mol/dm^{3} in 2
× 10^{4} sec. The rate constant of reaction in sec^{–1 }is : [JEE SCR 2003]
The reaction, X → Product follows first order kinetics. In 40 minutes the concentration of X changes from 0.1 M to 0.025 M. Then the rate of reaction when concentration of X is 0.01 M [JEE SCR 2004]
Which of the following statement is incorrect about order of reaction ? [JEE 2005]
Consider a reaction aG + bH → Products. When concentration of both the reactants G and H is doubled, the rate increases by eight times. However, when concentration of G is doubled keeping the concentration of H fixed, the rate is doubled. The overall order of the reaction is [JEE 2006]
Under the same reaction conditions, initial concentration of 1.386 mol dm^{–3} of a substance becomes
half in 40 seconds and 20 seconds through first order and zero order kinetics, respectively.
Ratio of the rate constants for first order (k_{1}) and zero order (k_{0}) of the reactions is [JEE 2008]
For a first order reaction A → P, the temperature (T) dependent rate constant (k) was found to follow the equation log k = – (2000) 1/T + 6.0. The preexponential factor A and the activation energy E_{a}, respectively, are [JEE 2009]
For the first order reaction
2N_{2}O_{5}(g) → 4NO_{2}(g) + O_{2}(g) [JEE 2011]
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