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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=5.20x10-3 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                           ?

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Answer #1

General guidance

Concepts and reason

This problem is based on the concept of chemical kinetics.

The rate of a chemical reaction is product of rate constant and concentration of reactants. In the mechanism of a chemical reaction, the slowest step is the rate determining step.

Fundamentals

For the reaction,

A+B\u2192C+D{\\rm{A}} + {\\rm{B}} \\to {\\rm{C}} + {\\rm{D}}

The rate of the reaction is written as follows:

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

Here, [A]\\left[ A \\right], [B]\\left[ B \\right] are the molar concentration of reactants A and B respectively.

Step-by-step

Step 1 of 3

(1)

The reaction is as follows:

C2H4Br2(aq)+3I\u2212(aq)\u2192C2H4(g)+2Br\u2212(aq)+I3\u2212(aq){{\\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)

Thus, the rate of reaction is written as follows:

r=k[C2H4Br2][I\u2212]r = k\\left[ {{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}} \\right]\\left[ {{{\\rm{I}}^ - }} \\right]

Substitute 0.00124Ms\u221210.00124{\\rm{ M }}{{\\rm{s}}^{ - 1}} for r, 5.20\u00d710\u22123M\u22121s\u221215.20 \\times {10^{ - 3}}{\\rm{ }}{{\\rm{M}}^{ - 1}}{\\rm{ }}{{\\rm{s}}^{ - 1}} for k and 0.244 M for [I\u2212]\\left[ {{{\\rm{I}}^ - }} \\right].

0.00124Ms\u22121=(5.20\u00d710\u22123M\u22121s\u22121)[C2H4Br2](0.244M)[C2H4Br2]=0.00124Ms\u22121(5.20\u00d710\u22123M\u22121s\u22121)(0.244M)=0.977M\\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 [C2H4Br2]\\left[ {{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}} \\right] is 0.977 M.


Explanation | Hint for next step

The initial concentration of the reactant is calculated by writing the rate law of the reaction.

Step 2 of 3

(2)

The reaction is as follows:

C2H4Br2(aq)+3I\u2212(aq)\u2192C2H4(g)+2Br\u2212(aq)+I3\u2212(aq){{\\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)

Thus, the rate of reaction is written as follows:

r=k[C2H4Br2][I\u2212]r = k\\left[ {{{\\rm{C}}_2}{{\\rm{H}}_4}{\\rm{B}}{{\\rm{r}}_2}} \\right]\\left[ {{{\\rm{I}}^ - }} \\right]

Substitute 0.000619Ms\u221210.000619{\\rm{ M }}{{\\rm{s}}^{ - 1}}

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