04-11-2018, 02:56 PM

Hi there,

I'm trying to do a rate of reaction problem I found online and am not getting the same answer as the one that is shown.

This is the reaction:

2 AB(g) → A2(g) +B2(g).

Time (s)

1. 0

2. 1000

3. 2000

4. 3000

5. 4000

[AB] (mol/L)

1. 1.00

2. 0.112

3. 0.061

4. 0.041

5. 0.031

So, they want me to find the kinetic constant for the rate of disappearance of AB. It would seem to be an order 2 reaction. Since the formula that gives rate of reaction is:

(dC/dt) = k(initial C of AB)^order

I did:

(0.969/4000)=k(1)^2

k = 2.4 x 10^-4

But apparently the right answer was supposed to be k = 3.9·10-3

Any help would be greatly appreciated.

I'm trying to do a rate of reaction problem I found online and am not getting the same answer as the one that is shown.

This is the reaction:

2 AB(g) → A2(g) +B2(g).

Time (s)

1. 0

2. 1000

3. 2000

4. 3000

5. 4000

[AB] (mol/L)

1. 1.00

2. 0.112

3. 0.061

4. 0.041

5. 0.031

So, they want me to find the kinetic constant for the rate of disappearance of AB. It would seem to be an order 2 reaction. Since the formula that gives rate of reaction is:

(dC/dt) = k(initial C of AB)^order

I did:

(0.969/4000)=k(1)^2

k = 2.4 x 10^-4

But apparently the right answer was supposed to be k = 3.9·10-3

Any help would be greatly appreciated.