Question
$2.00 Integrated Rate Law (2 questions) 1st order vs 2nd order
- From Chemistry: Inorganic-Chemistry
- Closed, but you can still post tutorials
- Due on Jul. 06, 2011
- Asked on Jul 03, 2011 at 12:07:05PM
Q:
When do you use integrated rate equation (1st order) and when do you use integrated rate equation (2nd order)?
Question 1. N2O5 (g)-->N2O4 (g) + 1/2O2 (g). If 2.50moles of N2O5 (g) are placed in a 5.00L container, how many moles of N2O5 would remain after 1.00minute? K=1.68x10^-2s^-1. Question 2. 2NOBr (g)-->2NO (g) + Br2 (g). K=0.810L/mol*sec. If there is an initial concentration of NOBr=4.00x10^-3M, how many seconds does it take to use up 1.50x10^-3M NOBr?
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here are your answers A++++
- This tutorial hasn't been purchased yet.
- Posted on Jul 03, 2011 at 12:45:45PM
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A:
Preview: ... 0.91 ...
The full tutorial is about 4 words long .
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correct answer
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- Posted on Jul 03, 2011 at 12:46:56PM
A:
Preview: ... (g)
according to integrated rate equation (2nd order)
k=0.810l/mol*sec
1/1.50x10^-3 ...
The full tutorial is about 27 words long .
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Step by Step Tutorial for your Questions A+
- This tutorial was purchased 1 time and rated No Rating by students like you.
- Posted on Jul 03, 2011 at 12:56:25PM
A:
Preview: ... when the ln[A] vs time for a reaction shows a linear graph. Use the 2 nd order integrated rate equation when 1/[A] vs time shows a linear graph. Basically, you are looking for a direct relationship with a linear graph, and integrated rate equations are based on direct relationships.
The reaction in Question 1 is 1 st order.
For N2O5 (g)-->N2O4 (g) + 1/2O2 (g)
The ...
The full tutorial is about 280 words long plus attachments.
Step by Step Tutorial A+++ for your questions.pdf (53K)