Could someone help me with this problem? I'm not really sure where to start. Thanks!
Dinitrogen pentoxide, N2O5, decomposes by first‑order kinetics with a rate constant of 3.7×10−5 s−1 at 298 K.
What is the half‑life, in hours, of N2O5 at 298 K?
Sapling #11 week 9/10
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Re: Sapling #11 week 9/10
Hi, so we know that this reaction is a first-order reaction so we can use the equation:
t1/2 = 0.693/k
Now, we need to input the rate constant, k, to find the half life (t1/2). Once you find the half-life, the units will be in seconds so we have to convert it to hours.
Hope this helps!
t1/2 = 0.693/k
Now, we need to input the rate constant, k, to find the half life (t1/2). Once you find the half-life, the units will be in seconds so we have to convert it to hours.
Hope this helps!
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Re: Sapling #11 week 9/10
The problem tells you the reaction is first order. So you use the first order half life equation to find the time, and convert it to hours.
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Re: Sapling #11 week 9/10
I agree with the previous posts! Since the question states that the reaction is first order, you would plug it into t1/2= ln2/k, where k is 3.7×10−5 s−1. Be sure to convert to hours after you find your answer!
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Re: Sapling #11 week 9/10
We use the equations t1/2=0.0693/k and then use the equation ln[A]-ln[A]0/-k=t to solve this question.
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Re: Sapling #11 week 9/10
i agree with above statements! It states in the question that it's a first order reaction, so we take the equation for a half life first order reaction.
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