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Consider the reaction described by the following equation what are the MISSING entries

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Question “Consider the reaction described by the following equation what are the MISSING entries”

Consider the reaction described by the following equation:

C2H4Br2(aq) + 3I- (aq) —–> c2H4 (g) + 2Br- (aq) + I3-
(aq)

rate= k{C2H4Br2}{I-} where k=5.20×10-3 M-1xs-1

What are the missing entries in the table?

Run           
[C2H4Br2]0 (M)       
[I-]0M              
Initial rate of formation of C2H4 (Mxs-1)

1                         
?                     
0.244                    
0.00124

2                       
0.244                   
?                        
0.000619

3                       
0.244                
0.244                          
?

Answer

General guidance

Concepts and Reason

This problem is based upon the concept of chemical Kinetics.

Rate constant and concentration of reactants determine the rate of chemical reactions. The rate determining step is the slowest in the chemical reaction mechanism.

Fundamentals

The reaction is here

{\\rm{A}} + {\\rm{B}} \\to {\\rm{C}} + {\\rm{D}}

This is how the rate of reaction is expressed:

r = k{\\left[ A \\right]^x}{\\left[ B \\right]^y}

Here, \\left[ A \\right]

Step-by-step

Step 1 from 3


(1)

This is the reaction:

{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}\\left( {aq} \\right) + 3{{\\rm{I}}^ - }\\left( {aq} \\right) \\to {{\\rm{C}}_2}{{\\rm{H}}_4}\\left( g \\right) + 2{\\rm{B}}{{\\rm{r}}^ - }\\left( {aq} \\right) + {{\\rm{I}}^{3 - }}\\left( {aq} \\right)

The rate of reaction can be summed up as follows:

r = k\\left[ {{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}} \\right]\\left[ {{{\\rm{I}}^ - }} \\right]

Substitute $math_tag_5

\\begin{array}{c}\\\\0.00124{\\rm{ M }}{{\\rm{s}}^{ - 1}} = \\left( {5.20 \\times {{10}^{ - 3}}{\\rm{ }}{{\\rm{M}}^{ - 1}}{\\rm{ }}{{\\rm{s}}^{ - 1}}} \\right)\\left[ {{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}} \\right]\\left( {0.244{\\rm{ M}}} \\right)\\\\\\\\\\left[ {{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}} \\right] = \\frac{{0.00124{\\rm{ M }}{{\\rm{s}}^{ - 1}}}}{{\\left( {5.20 \\times {{10}^{ - 3}}{\\rm{ }}{{\\rm{M}}^{ - 1}}{\\rm{ }}{{\\rm{s}}^{ - 1}}} \\right)\\left( {0.244{\\rm{ M}}} \\right)}}\\\\\\\\ = 0.977{\\rm{ M}}\\\\\\end{array}

Part 1

The value of $math_tag_7


Hint for next step

By writing the rate law for the reaction, the initial concentration of reactant can be calculated.

Step 2 from 3


(2)

This is the reaction:

{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}\\left( {aq} \\right) + 3{{\\rm{I}}^ - }\\left( {aq} \\right) \\to {{\\rm{C}}_2}{{\\rm{H}}_4}\\left( g \\right) + 2{\\rm{B}}{{\\rm{r}}^ - }\\left( {aq} \\right) + {{\\rm{I}}^{3 - }}\\left( {aq} \\right)

The rate of reaction can be summed up as follows:

r = k\\left[ {{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}} \\right]\\left[ {{{\\rm{I}}^ - }} \\right]

Substitute $math_tag_10

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