Question

At 3500 K, the following reaction has the rate law Rate = k[H2][Ar], where k =...

At 3500 K, the following reaction has the rate law Rate = k[H2][Ar], where k = 2.2 x 10^5 M^-1sec^-1

H2(g) + Ar(g) → 2 H(g) + Ar(g)

a. Calculate the rate of reaction when [H2] = 1.0 x 10^-3 M and [Ar] = 7.2x 10^-4 M.

b. Derive an expression for t½ for a second order reaction (Rate = k[A]^2).

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
During the initial stages of the following reaction the rate law is Rate = k[H2][Br2]½. H2(g)...
During the initial stages of the following reaction the rate law is Rate = k[H2][Br2]½. H2(g) + Br2(g) → 2 HBr(g) What is the order of the reaction with respect to each component and the overall order?
H2O2 decomposes at 20˚C in a first order reaction where k = 1.06 x 10-3min-1. If...
H2O2 decomposes at 20˚C in a first order reaction where k = 1.06 x 10-3min-1. If the initial concentration of H2O2 is 0.020 M, what is [H2O2] after 3.5 days? a. 9.6x10-5 M b. 5.1x10-5 M c. 4.4x10-5 M d. 1.7x10-5 M For the following reaction, calculate the average reaction rate over the last 2 minutes using the table of data below. H2(g)   +   2ICl(g)      I2(g)   +   2HCl(g) Time (min)     [ICl] (M) --------------     -----------         0             2.000         2            ...
Determine the rate law and the value of k for the following reaction using the data...
Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.093 4.84 x 10-4 0.084 4.37 x 10-4 0.224 1.16 x 10-3 Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.093 4.84 x 10-4 0.084 4.37 x 10-4...
at 300 K the reaction below obeys the rate law rate=k[NOCl]2 where k= 2.8x10-5 M-1* S-1...
at 300 K the reaction below obeys the rate law rate=k[NOCl]2 where k= 2.8x10-5 M-1* S-1 2NOCl ------> 2NO + Cl2 Suppose 1.0 mole of NOCl is introduced into a 2.0- liter container at 300 k. How much NOCl will remain after 30 minutes? the answer is 0.95 mol but how do you get this?
The experimentally determined rate law for the reaction 2NO(g)+2H2(g)→N2(g)+2H2O(g) is rate=k[NO]2[H2]. Part A What are the...
The experimentally determined rate law for the reaction 2NO(g)+2H2(g)→N2(g)+2H2O(g) is rate=k[NO]2[H2]. Part A What are the reaction orders in this rate law? Enter your answers numerically separated by commas. nNO, nH2 = SubmitMy AnswersGive Up Part B Would the reaction rate increase more if we double the concentration of NO or the concentration of H2? A) The reaction rate will increase more if we double the concentration of NO. B) The reaction rate will increase more if we double the...
A packed bed reactor has the reaction A --> B occurring. The rate law is –rA...
A packed bed reactor has the reaction A --> B occurring. The rate law is –rA = kCA where k = 15 L/g-min. The superficial gas velocity is 4.8 kg/m2-s with a density of 0.45 kg/m3 and a viscosity of 3.9x10-5 kg/m-s. The porosity, catalyst density, and particle diameter are, respectively, 0.45, 2.2 g/cm3 and 0.255 cm. The cross sectional area of the reactor is 12 cm2. The inlet pressure is 100 kPa. Calculate the conversion ‘X’ when the catalyst...
1) If the rate law for the clock reaction is:     Rate = k [ I-]...
1) If the rate law for the clock reaction is:     Rate = k [ I-] [ BrO3-] [H+] A clock reaction is run with the following initial concentrations: [I-]               [BrO3-]            [H+]                         [S2O32-] 0.002                   0.008                   0.02                          0.0001   The reaction time is 29 seconds Calculate k in the rate law: 2)If the rate law for the clock reaction is:     Rate = k [ I-] [ BrO3-] [H+] A clock reaction is run...
Determine the rate law (be sure to include the value for k) for the following reaction...
Determine the rate law (be sure to include the value for k) for the following reaction using the data provided. NO2(g)+O3(g)->NO3(g)+O2(g) [NO2] (M) [O3]i (M) initial rate 0.10 0.33 0.0223 0.10 0.66 0.01788 0.25 0.66 1.112 Please help with reasoning on how to find the order of the reactions when they are not first or 0 order and how to find k. Thank you!
The rate law for the reaction: 2H2+2NO--->N2+2H2O is rate=k[H2][NO]^2. Which of the follwing mechanisms can be...
The rate law for the reaction: 2H2+2NO--->N2+2H2O is rate=k[H2][NO]^2. Which of the follwing mechanisms can be ruled out on the basis of the observed rate expression? PLEASE EXPLAIN Mechanism 1: H2+NO--->H2O+N (slow) / N+NO----->N2+O (fast) / O+H2----> N2+O (fast) Mechanism 2: H2+2NO---->N2O+H2O (slow) / N2O+H2---->N2+H2O (fast) Mechanism 3: 2NO<----->N2O2 (fast equilibrium) / N2O2+H2------>N2O+H2O (slow) / N2O+H2------>N2+H2O (fast) PLEASE EXPLAIN WHY.
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) +...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g) forward and reverse arrows 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.383 moles kf H2 and 0.383 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M [I2] = M [HI] = M
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT