Consider the reaction
                        3A + B + C - D + E
            where the rate law is defined as
                        Rate = k [A] 2 [B][C]
            An experiment is carried out where [B] 0 = [C] 0 = 1.00 M and [A] 0 = 1.00 x 10 –4 M.

After 3.00 minutes, [A] = 3.26 x 10 –5 M. The value of k is

Question

Consider the reaction 
                         3A + B + C  ->  D + E 
             where the rate law is defined as 
                         Rate  =  k [A] 2 [B][C] 
             An experiment is carried out where [B] 0  = [C] 0  = 1.00 M and [A] 0  = 1.00  x  10 –4  M. 
   
 After 3.00 minutes, [A] = 3.26 x  10 –5  M. The value of  k  is

Answer

none of these

Answer

1.00  x  10 8  L 3 /mol 3  .s

Answer

3.26  x  10 –5  L 3 /mol 3  .s

Answer

1.15  x  10 2  L 3 /mol 3  .s

Answer

6.23  x  10 –3  L 3 /mol 3  .s

Crowdly

Consider the reaction 3A + B + C -> D + E ...

Want instant access to all verified answers on elearn.squ.edu.om?