Question

Consider the reaction described by the following equation.

C2H4Br2(aq)+3I^-(aq) ----->  C2H4(g)+2Br^-(aq)+i(negative charge)(three subscript) (aq)

The rate law is

rate = k[C2H4Br2] [I^-]        Where k=5.90x10^-3 M^-1 s^-1

What are the missing entries in the following table?

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

_____________________________________________________

1                x                        0.242          0.00138

2                0.242                 y                 0.000691

3                0.242                 0.242          z

x=_____M     y=_________M       z=________M s^-1

Answer 1

For x value:

To find this value you can write the rate law in this way:

x=[C2H4Br2] = v / k[I-]

Taking the other values that we have in the table you can obtain x:

x = (0.00138 M/s)/(5,9 x 10^-3M^-1s^-1)(0.242 M) = 0,967 M

For y value:

To find this value you can write the rate law in this way:

y=[I-] = v/k[C2H4Br2]

Replacing the values in the table:

y = (0.00691 M/s)/(5.9 x 10^-3M^-1s^-1)(0.242 M) = 4.84 M

And for the z value you replace the values that are in the table directly in the rate law:

z=v=(5,9 x 10^-3M^-1s^-1)(0.242 M)(0.242 M) = 0.346 M/s