The initial rates listed in the following table were determined forthe reaction

Question

The initial rates listed in the following table were determined forthe reaction
2NO(g)+Cl2(g)>>2NOCl(g)

Experiment Initial (NO) Initial (Cl2) Initial Rate of Consumption of Cl2 (M/s)
------(1)-------------(0.13)---------(0.20)------------------(1.0*10^-2)------------
------(2)-------------(0.26)---------(0.20)------------------(4.0*10^-2)------------
------(3)-------------(0.13)---------(0.10)------------------(5.0*10^-3)------------

Part A
What is the rate law?
Rate=k[NO]^2[Cl2]


Part B
What is the value of the rate constant?
k=____________________________ /M^2*s


Part C
What is the initial rate when the initial concentrations of both reactants are 0.15 M ?
Rate=__________________________M/s

Explanation / Answer

After solving (A) you get rate law is , rate , r = k [NO] 2 [Cl2 ]    ----(1) Take the 1st values of the given table that [ NO] = 0.13 M                                                                [ Cl2 ] = 0.20 M                                                                rate , r = 1.0 x 10 -2 M/s Plug the values in (1) we get k = r / (  [NO] 2 [Cl2 ] )                                                = 1.0 x 10 -2 / ( 0.13 2 x 0.20 )                                                = 2.958 M -2 s -1 Part C :- ------- What is the initial rate when the initial concentrations of both reactants are 0.16 M r = k [NO] 2 [Cl2 ] = 2.958 M -2 s -1 x 0.16 2 x 0.16 = 0.0121 M/s

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