Chemistry Homework Solutions
#188426
Rate Constant for a Second-Order Reaction
The rate constant for the second-order reaction given below is 0.80/M·s at 10°C.
2 NOBr(g) ----> 2 NO(g) + Br2(g)
(a) Starting with a concentration of 0.080 M, calculate the concentration of NOBr after 13 s.
(b) Calculate the half-life when [NOBr]0 = 0.090 M.
(c) Find the half-life when [NOBr]0 = 0.044 M
The solution is comprised of detailed explanations of rate law for second order reaction.
What is this?
By OTA - Overall OTA Rating
Yanfang Li, PhD - 4.9/5
Purchase Cost Now
$2.19 CAD (was ~$3.99)
Included in Download
- Plain text response
Why you can trust BrainMass.com
- Your Information is Secure
- Best Online Academic Help Service
- Students find real academic Success
- Integrated Law for Reaction - The reaction A produces B + C is known to be zero order in A and to have a rate constant of 5.0 x 10 superscript-2 mol/L x sec. @ 25 degrees C. An experiment was run at 25 degrees C where [A]0 = 1.0 x ...
- Multiple choice question about half lives and rate constants. - What is the half-life for a first order reaction with a rate constant of 0.573s(to the negative 1)? a. 1.21s b. 0.827s c. 1.25s d. 0.278s e. 3.49s
- Rate constant for a second order reaction - The rate constant for the second-order reaction is 0.80/M*s at 10 degrees C 2NOBr(g) goes to 2NO(g) + Br2 (g) (a) Starting with a concentration of 0.071 M, calculate the ...
- Using experimental results to determine the order of a chemical reaction and the rate constant from your understanding of chemical kinetics and species half life. - A reaction is defined by the following scheme: X à Y When the concentration of X in a solution is 1.02 M, the half-life (t1/2) is 160 seconds. When the concentration of X in solution is 2.05 ...
- oxidation - Questions 17 - 18: Hsub3AsOsub4 + 3I^- + 2Hsub3O^+ -> Hsub3AsOsub3 + Isub3^- + 3Hsub2O The oxidation of iodide ions by arsenic acid in acidic aqueous solution occured accoring to the balanced ...
