In a reaction involving the bromination of acetone, the following initial concentraions were present in the reaction mixture.
acetone (0.8mol/L), H+ (0.2 mol/L), Br2 (0.004 mol/L)
At 25 degrees C, it took 240s before the colour of Br2 disappeared. If the reaction is zero order in Br2, how long would it take for the Br2 to react if the initial Br2 concentration was 0.008 mol/L and all the other conditions remained the same??
Help!
I thought zero order meant that the reaction did NOT depend upon initial concn (as long as there is some present).
So the rate would not change, right?
http://en.wikipedia.org/wiki/Rate_equation
To solve this problem, we need to understand the concept of reaction orders and how they affect the rate of a chemical reaction.
In this case, you are given that the bromination of acetone is a zero-order reaction with respect to Br2. This means that the rate of the reaction does not depend on the concentration of Br2.
Since we know the reaction is zero order with respect to Br2, we can assume that doubling the concentration of Br2 will double the rate of the reaction.
From the given data, we know that it took 240 seconds (s) for the color of Br2 to disappear when the initial Br2 concentration was 0.004 mol/L.
To find how long it would take for the Br2 to react if the initial Br2 concentration is 0.008 mol/L, we can set up a proportion:
(time 1) / (concentration 1) = (time 2) / (concentration 2)
240 s / 0.004 mol/L = (time 2) / 0.008 mol/L
Solving for (time 2), we get:
(time 2) = (240 s * 0.008 mol/L) / 0.004 mol/L
(time 2) = 480 s
Therefore, if the initial Br2 concentration is 0.008 mol/L and all the other conditions remain the same, it would take 480 seconds for the Br2 to react.