In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture:
10 mL 4.0 M acetone + 10mL 1.0 M HCL + 10 mL 0.0050 M I2 + 20 mL H2O
A student found that it took 250 seconds for the color of the I2 to disappear. What was the rate of the reaction?
this not helping, i need to know how to do it
To find the rate of the reaction, we need to calculate the change in concentration of iodine per unit time. The rate of the reaction can be determined by using the formula:
Rate = Δ[I2] / Δt
In this case, we know the initial concentration of iodine ([I2]0) is 0.0050 M and the final concentration of iodine ([I2]) after it disappears completely is 0 M.
First, we need to calculate the change in concentration of iodine, which is:
Δ[I2] = [I2] - [I2]0
Δ[I2] = 0 M - 0.0050 M
Δ[I2] = -0.0050 M
Next, we need to calculate the change in time, which is:
Δt = final time - initial time
= 250 s - 0 s
= 250 s
Finally, we can substitute the values into the rate formula:
Rate = Δ[I2] / Δt
Rate = (-0.0050 M) / (250 s)
Now we can calculate the rate of the reaction:
Rate = -0.0050 M / 250 s
Rate = -0.00002 M/s
Therefore, the rate of the reaction is -0.00002 M/s, indicating that the concentration of iodine is decreasing by 0.00002 M per second.