Chemical Kinetics - Initial Rates Method
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- Опубликовано: 8 июл 2024
- This chemistry video tutorial provides a basic introduction into chemical kinetics. It explains how to calculate the average rate of disappearance of a reactant as well as how to identify the rate law expression using the initial rates method. It explains how to calculate the rate constant along with the appropriate units and how to calculate the initial rate of the reaction given the concentration of the reactants.
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14:30, the answer supposed to be positive because [NO] is decreasing with time therefore we're supposed to multiply -8.2 x 10³ m/s with a negative sign (-), inclusion the final answer is 8.2 x 10³. Look it up in Zuhmdahl 9th Ed, page 555-556
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14:19 Why didn't you multiply by 1/2 since the coefficient of NO is 2?
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At 14:23, wouldn't you need to add the (1/2) in front of your calculation given that the coefficient of NO is 2?
I came through the comment section for this but couldnt find the answer either
The problem asks for the average rate of disappearance of NO in the first 20 seconds. The average rate of disappearence is defined as -Δ[R]/Δt, where Δ[R] is the change in concentration of the reactant.
The reason you don't divide by the coefficient is because that would give you the average reaction rate (Rate = 1/2 (-Δ[NO]/Δt)), not the average rate of disappearence of NO.
Therefore, for NO, -(0,586 - 0,750) M / 20 s is the final answer, which should be positive, not negative like in the video.
Also I believe there is a mistake in the chemical equation (although it doesn't matter for this problem), the product of this reaction should be 2NO₂, not 2NO.
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at 14:27, why don't you take into account the 1/2 since we're looking for the rate? aren't you supposed to multiply that by the change in NO over time?
i asked my chem prof this and she said that if it's just 1 reaction then you would use the idea that he did but he didnt clarify this lol. in real problems, you have to use the 1/coefficient rule
It is cause we are finding rate of dissaperance of NO instead of rate of the reaction where we have to use 1/coefficient
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