Consider the reaction described by the following equation. C2H4Br2(aq)+3I^-(aq)
ID: 810767 • Letter: C
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
Explanation / Answer
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