The following data was collected for the rate of dissapearanceof CO in the react

Question

The following data was collected for the rate of dissapearanceof CO in the reaction: 2 CO (g) + O2 (g) -->CO2. Experiment [CO] (M) [ O2] (M) Initial Rate (M/s) 1 0.0312 0.0068 1.41 x 10-2 2 0.0624 0.0068 5.64 x 10-2 3 0.0624 0.0136 1.13 x 10-1 (a) What is the rate law for the reaction? (b) What is the overall order of the reaction? (c) What are the units of the rate constant? (d) What is the value of the rate constant? (e) What is the rate of dissapearance of CO when [CO] =0.0750M and [O2] = 0.0250M? The following data was collected for the rate of dissapearanceof CO in the reaction: 2 CO (g) + O2 (g) -->CO2. Experiment [CO] (M) [ O2] (M) Initial Rate (M/s) 1 0.0312 0.0068 1.41 x 10-2 2 0.0624 0.0068 5.64 x 10-2 3 0.0624 0.0136 1.13 x 10-1 (a) What is the rate law for the reaction? (b) What is the overall order of the reaction? (c) What are the units of the rate constant? (d) What is the value of the rate constant? (e) What is the rate of dissapearance of CO when [CO] =0.0750M and [O2] = 0.0250M? Experiment [CO] (M) [ O2] (M) Initial Rate (M/s) 1 0.0312 0.0068 1.41 x 10-2 2 0.0624 0.0068 5.64 x 10-2 3 0.0624 0.0136 1.13 x 10-1

Explanation / Answer

a)Expt 3 / Expt2 = ( 0.0136 / 0.0068 )y                        = ( 1.13 x 10-1 M /s / 5.64 x 10-2M/s)                        = (2)               (2)y  = (2)                y     = 1 Expt 2 / Expt 1  = (5.64 x 10-2 M/s /1.41 x 10-2 M/s)                                 = ( 0.0624 / 0.0312 )x
                 (2)x     = (4)                         = (2)2                    x   = 2 rate = k [CO]2[O2]                    x   = 2 rate = k [CO]2[O2] b) Overall order of the reaction is 3. c) units of rate constant k = rate / [CO]2[O2]                                        =M /s / (M)2(M)                                       = L2 / M2 .s d) k = 1.41 x 10-2 mol / L / ( 0.0312 M)2 ( 0.0068 M)          =2130 L2 / M2 .s e) rate =  2130 L2 / M2.s * ( 0.0750 M) 2(0.0250 M)            = 0.299 M/s e) rate =  2130 L2 / M2.s * ( 0.0750 M) 2(0.0250 M)            = 0.299 M/s

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