Dinitrogen pentoxide decomposes via a first order reaction. Rate = k[N,O5], k= 6.93 × 10-3 s-1 The concentration of N,O5 is initially 0.700 mol/L. After 100 s it has dropped to 0.350 mol/L and after 200 s it has dropped to 0.175 mol/L. What is the concentration after 150 s? HOW DO WE GET THERE? Use the first order concentration-time equation to determine [N2O5] remaining after 150 s. [N2O5] = 150 X mol/L

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INTERACTIVE EXAMPLE First Order Rate Laws: Concentration vs. Time
Dinitrogen pentoxide decomposes via a first order reaction.
Rate = k[N2O5], k= 6.93 × 10-3 s-1
The concentration of N,O5 is initially 0.700 mol/L. After 100 s it has dropped to 0.350 mol/L and after 200 s it has
dropped to 0.175 mol/L. What is the concentration after 150 s?
HOW DO WE GET THERE?
Use the first order concentration-time equation to determine [N2O5] remaining after 150 s.
[N205] = 150
X mol/L
Transcribed Image Text:[References] INTERACTIVE EXAMPLE First Order Rate Laws: Concentration vs. Time Dinitrogen pentoxide decomposes via a first order reaction. Rate = k[N2O5], k= 6.93 × 10-3 s-1 The concentration of N,O5 is initially 0.700 mol/L. After 100 s it has dropped to 0.350 mol/L and after 200 s it has dropped to 0.175 mol/L. What is the concentration after 150 s? HOW DO WE GET THERE? Use the first order concentration-time equation to determine [N2O5] remaining after 150 s. [N205] = 150 X mol/L
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