Reaction Rates
The equation for the reaction of ICl and H2 is shown below.
2ICl (g) + H2(g) → 2HCl (g) + I2(g)
The rate constant k for this reaction is 1.63 × 10−6 dm3 mol−1 s−1.
What is the overall order of the reaction?
A 0
B 1
C 2
D 3
I understand that you have to use the units but how?
2ICl (g) + H2(g) → 2HCl (g) + I2(g)
The rate constant k for this reaction is 1.63 × 10−6 dm3 mol−1 s−1.
What is the overall order of the reaction?
A 0
B 1
C 2
D 3
I understand that you have to use the units but how?
(edited 7 months ago)
Original post by Incrediblezed
The equation for the reaction of ICl and H2 is shown below.
2ICl (g) + H2(g) → 2HCl (g) + I2(g)
The rate constant k for this reaction is 1.63 × 10−6 dm3 mol−1 s−1.
What is the overall order of the reaction?
A 0
B 1
C 2
D 3
I understand that you have to use the units but how?
2ICl (g) + H2(g) → 2HCl (g) + I2(g)
The rate constant k for this reaction is 1.63 × 10−6 dm3 mol−1 s−1.
What is the overall order of the reaction?
A 0
B 1
C 2
D 3
I understand that you have to use the units but how?
The rate of a chemical reaction is always measured in mol dm^-3 s^-1.
If you divide the units of the rate of a chemical reaction by the units of its rate constant, you will always get the units of concentration (mol dm^-3) raised to the power of the overall reaction order.
See what happens when you try this approach.
(edited 7 months ago)
Original post by Incrediblezed
The equation for the reaction of ICl and H2 is shown below.
2ICl (g) + H2(g) → 2HCl (g) + I2(g)
The rate constant k for this reaction is 1.63 × 10−6 dm3 mol−1 s−1.
What is the overall order of the reaction?
A 0
B 1
C 2
D 3
I understand that you have to use the units but how?
2ICl (g) + H2(g) → 2HCl (g) + I2(g)
The rate constant k for this reaction is 1.63 × 10−6 dm3 mol−1 s−1.
What is the overall order of the reaction?
A 0
B 1
C 2
D 3
I understand that you have to use the units but how?
k = Rate/[A]
k = dm3 mol-1 s-1
Rate = mol dm-3 s-1
Overall order = Rate / k
If you compare the units you realise overall order = 2
Original post by PixiePresents
k = Rate/[A]
k = dm3 mol-1 s-1
Rate = mol dm-3 s-1
Overall order = Rate / k
If you compare the units you realise overall order = 2
k = dm3 mol-1 s-1
Rate = mol dm-3 s-1
Overall order = Rate / k
If you compare the units you realise overall order = 2
OHH okay thanks I understand now
Hi @Incrediblezed,
I've updated the title of your thread to "Reaction Rates" and added an A-Level label for better clarity. While you did receive responses, it's advisable to be more specific in your query to receive a faster response.
Wishing you an excellent weekend, and please don't hesitate to ask if you have any further questions or if anything else is unclear.
5hyl33n
I've updated the title of your thread to "Reaction Rates" and added an A-Level label for better clarity. While you did receive responses, it's advisable to be more specific in your query to receive a faster response.
Wishing you an excellent weekend, and please don't hesitate to ask if you have any further questions or if anything else is unclear.
5hyl33n
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