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In the reaction:A + 2B→ 3C+D ,which of the following expression does not described change in the concentration of various species as a function of time?
For the given reaction.
The accompanying figure depicts the change in concentration of species X and Y for the reaction , as a function of time. The point of intersection of the two curves represnts.
The intersection point indicates that half of the reactant X is converted into Y.
In a reaction, the rate expression is, rate = K [A] [B] ^{2/3} [C] ^{0}, the order of reaction is:
Order of reaction is sum of powers raised on concentration terms in order to write rate expression.
For a reversible reaction A B, Ist order in both the directions, the rate of reaction is given by:
Rate = K_{1}[A]K_{2}[B] for a reversible reaction of 1 order opposed by 1 order.
For zero order reaction
On intergrating, [A] = Kt + c
or y = c + mx
For the decomposition of N_{2}O_{5}(g), it is given that:
Activation energy E_{a}
_{}
Activation energy E'_{a}
_{then:}
Energy of activation does not depend on the stoichiometry of change. It is characteristic value for a chemical reaction.
A reaction, occurs by the following mechanisum :
A_{2 }⇆ A + A .......(Slow)
Its order would be:
rate = K[ A_{2}]
The rate of reaction becomes 2 times for every 10^{0}C rise in temperature. How the rate of reaction will increase when temperature is increased from 30^{0}C to 80^{0}C?
rate_{2 = x rate , the rate increases by 25 times, i.e., 32 times. }
A drop of solution (volume 0.05 mL) contains 3.0 x 10^{6} mole of H^{+}. If the rate constant of disappearance of H^{+} is 1.0 x 10^{7} mol litre^{1} sec^{1}. How long would it take for H^{+} in drop to disappear?
Since rate constant = 1 x 10^{7} mol litre^{1} sec^{1}
∴ Zero order reaction
0.05 mL has 3 x 10^{6} mole of H^{+}
Ethylene is produced by cyclobutane as:
The rate constant is 2.48 x 10^{4} sec^{1}. In what time will the molar ratio of the ethylene to cyclobutane in reaction mixture attain the value equals to unity ?
Mole at t = 0 a 0
Mole at t = t (ax) 2x
=1635.2 second = 27.25 minute
A reaction takes place in three steps with individual rate constant and activation energy.
Overall rate constant, K = (k_{1}k_{3}/k_{2})^{2/3}
Overall activation energy of the reaction will be:
= 2/3 [180 + 80  50] = 140KJ/mol
In the following first order competing reactions :
A + Reagent > Product
B + Reagent > Product
The ratio of K_{1}/K_{2}, if only 50% of B will have been reacted when 94% of A has been reacted in same time is:
For 50% B reacted, K_{2} = (2.303/T_{2})log100/50
For 94% A reacted, K_{1} = (2.303/T_{1})log100/6
K_{2}/K_{1} = t_{2}/t_{1}x0.3010/1.2218
Since t_{2} = t_{1}, because 50% B has reacted when 94% A has reacted.
K_{2}/K_{1} = 0.3010/1.2218 = 0.246 and K_{1}/K_{2} = 4.06
From the following data, the activation energy for the reaction (cal/mol):
A substance undergoes first order decomposition. The decomposition follows two parallel first order reactions as:
The percentage distribution of B and C are:
For parallel path reaction
Mathematical expression for t_{1/4,} i.e., when (1/4)th reaction is over following first order kinetics can be given by:
The rateconstant of a second order reaction is 10^{2} (Ms)^{1}. The rate constant expressed in cc. molecule^{1} min^{1} is:
K = 10^{2 }mol^{1 }litre sec^{1 }
The rate of disappearance of SO_{2} in the reaction; 2SO_{2} + O_{2} > 2SO_{3} is 1.28 x 10^{3 }g/sec. The the rate of formation of SO_{3} is:
The rate of formation of SO_{3} is 1.28×10^{−3}g/sec.
The rate of a first order reaction is 1.5 x 10^{2} M min1 at 0.5 M concentration of reactant. The halflife of reaction is:
For a reaction aA >bB when [A] = 2.2 mM, the rate was found to be 2.4 mMs^{1}. On reducing concentration of [A] to half , the rate changes to 0.6 mMs^{1}. The order of reaction with respect to A is:
During the kinetic study of the reaction following results were obtained.
On the basis the data, which one is correct?
Use : r = K [ A ]^{m} [ B ]^{n}
The reaction L > 4 is started with 10 g of L. After 30 and 90 mintue, 5 g and 1.25 g of L are left respectively. The order of reaction is :
The given data suggests that which is obeyed by first order reaction.
The differential rate expression for the reaction H_{2} + I_{2 }> 2HI is:
follow review of rate of reaction.
In a first order reaction the concentration of reactant decreases from 800 mol/dm^{3} to 50 mol/dm^{3} in 2 x 10^{4} sec. The rate constant of reaction in sec1 is:
Plots showing the variation of the rate constant (k) with temperature (T) are given below. The plot that follows Arrhenius equation is:
i.e , K = increase exponentially, with rise in temperature.
The rate constants of three reactions involving reactant A only obeying I, II, III order respectively is same. Which of the following is true?
r_{1} = K [ A ]^{1} ; r_{2} = K [ A ]^{2} ; r_{3} = K [ A ]^{3}
log_{e} K vs. 1/T plots shows a straight line having slope of 120^{0} and intercepts on the Yaxis of 2, then :
A reaction occurs in three rate detemining steps having rate constant K_{1}, K_{2} and K_{3} respectively and arrehenius factor A_{1}, A_{2}, A_{3} respectively. The overall rate constant . If energy of activations for each step is Ea_{1}, Ea_{2}, and Ea_{3} respectively, then overall energy of activation is:
At 3 km altitude, water boils at 90^{0}C and 300 seconds are taken to cook a ‘3 minute egg’. The temperature coefficient for the process of cooking is:
Temperature coefficient
C is the correct answer.
According to Le Chatelier’s principle rate of exothermic reactions decreases with an increase in temperature.
The rate expression for a reaction is (α and β > 0). The half life of the reaction can be given by:
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