If N2O5 decomposes to NO2 and O2 in a 1st order rate with a constant of 4.8x10^-4/s at 45°C, if the initial concentration of N2O5 was 1.65x10^-7 mol/L, how long (in minutes) does it take to decrease the N2O5 concentration to 1.00x10^-2 mol/L?
Added by Randy H.
Step 1
00x10^-2 / 1.65x10^-7) = ln(6.06x10^4) = 11.01 Show more…
Show all steps
Your feedback will help us improve your experience
Dj Tan and 82 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 × 10^-4/s at 45°C. If the initial concentration of N2O5 is 7.98 × 10^-2 mol/L, what is the concentration of N2O5 after 503 s? How long would it take for the concentration of N2O5 to decrease to 1.00 × 10^-2 mol/L from an initial concentration of 7.98 × 10^-2 mol/L?
Madhur L.
The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 × 10^-4/s at 45°C. If the initial concentration of N2O5 is 2.12 × 10^-2 mol/L, what is the concentration of N2O5 after 504 s? How long would it take for the concentration of N2O5 to decrease to 1.00 × 10^-2 mol/L from an initial concentration of 2.12 × 10^-2 mol/L?
Adi S.
The decomposition of N2O5(g) ---> NO2(g) + NO3 (g) proceeds as a first order reaction with a half-life of 30.0 seconds at a certain temperature. If the initial concentration [N2O5]0 = 0.400 M, what is the rate constant of the reaction?
Krishna G.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD