Write a balanced reaction for which the following rate relationships are true. R
ID: 1013849 • Letter: W
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Write a balanced reaction for which the following rate relationships are true. Rate = 1/2 Delta [N_2]/Delta t = Delta [O_2]/Delta t = -1/2 Delta [N_2O]/Delta t 1/2 N_2 + O_2 rightarrow 1/2 N_2O N_2O rightarrow N_2 + 2 O_2 2 N_2O rightarrow 2 N_2 + O_2 1/2 N_2O rightarrow 1/2 N_2 + O_2 2 N_2 + O_2 rightarrow 2 N_2O Given the following balanced equation, determine the rate of reaction with respect to [O_2]. If the rate of formation of O_2 is 7.78 Times 10^-1 M/s, what is the rate of the loss of O_3? 2 O_3 (g) rightarrow 3 O_2(g) 1.17 M/s 0.519 M/s 2.34 M/s 7.78 M/s 1.56 M/s Give the characteristic of a second-order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant. The rate of the reaction is proportional to the square root of the concentration of the The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant. A rate is equal to 0:0200 M/s. If [A] = 0.100 M and rate = k[A][B]^2, what is the new rate if the concentration of [A] is increased to 0.200 M? 0.0200 M/s 0.0400 M/s 0.0600 M/s 0.0800 M/s 0.100 M/s What are the units of k in the following rate law? Rate = k [X] [Y]^3 1/M^3 s 1/M^2 s M/s 1/M sExplanation / Answer
(1) The balanced reaction is : 2N2O ---> 2N2 + O2
The rate of the reaction = rate of disappearance of reactants = rate of appearance of products
= (-1/2)d[N2O]/dt =(1/2) d[N2]/dt = d[O2]/dt
Therefore option (c) is correct.
(2) 2O3 ----> 3O2
The rate of the reaction = rate of disappearance of reactants = rate of appearance of products
= (-1/2)d[O3]/dt = (1/3) d[O2]/dt
Given rate of formation of O2 = d[O2]/dt = 7.78x10-1 M/s
rate of loose of O3 is = d[O3]/dt = (2/3) d[O2]/dt = (2/3) x 7.78x10-1 M/s = 0.519 M/s
(3) For a second order reaction the rate of the reaction is proportional to square of the concentration of the reactant.
So option (B) is correct
(4) Given rate , r = k[A][B]2
Given rate = 0.0200 M/s
[A] = 0.100 M
When the concentration of A increased to 0.200 M=2xA, then the new rate is r' =k[2A][B]2
= 2xk[A][B]2
= 2 x r
= 2x0.0200 M/s
= 0.0400 M/s
Therefore option (B) is correct
(5) Given rate = k[X][Y]3
The units of rate of reaction is M/s
The units of k are k = rate /([X][Y]3)
= (M/s) / (M x M3)
= 1 /(M3s)
Therefore option (A) is correct
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