Question

The reaction in which NO2 forms a dimer is second order in NO2 : 2NO2(g) --->...

The reaction in which NO2 forms a dimer is second order in NO2 :

2NO2(g) ---> N2O4(g) Rate = k [NO2]2

Calculate the rate constant for this reaction if it takes 0.0050 s for the initial concentration of NO2 to decrease from 0.50M to 0.25M.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The decomposition of NO2 2NO2(g) → 2NO(g) + O2(g) is second-order in NO2. Given that the...
The decomposition of NO2 2NO2(g) → 2NO(g) + O2(g) is second-order in NO2. Given that the half-life for the inital concentration of NO2 equal to 0.848 M is 221 s, find the concentration of NO2 after 663 s.
7. Consider the following reaction: 2NO2 (g) -> 2NO(g) + O2 (g) rate = k[NO2]^2 When...
7. Consider the following reaction: 2NO2 (g) -> 2NO(g) + O2 (g) rate = k[NO2]^2 When the initial concentration of NO2 is 100 mM, it takes 55 s for 90% of the NO2 to react. Calculate the rate constant. a) 0.042 M–1·s–1 d) 1.6 ´ 10–3 M–1·s–1 b) 1.8 ´ 10–5 M–1·s–1 e) 0.13 M–1·s–1 c) 1.6 M–1·s–1 I am getting d.) but i am not sure, please confirm
Consider the reaction 2NO2(g)?N2O4(g) Calculate ?G at 298 K if the partial pressures of NO2 and...
Consider the reaction 2NO2(g)?N2O4(g) Calculate ?G at 298 K if the partial pressures of NO2 and N2O4 are 0.38atm and 1.64atm , respectively.
For the following reaction, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a reaction...
For the following reaction, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a reaction vessel initially contains an N2O4 concentration of 5.50×10−2 MM at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K? [N2O4], [NO2] = nothing
Consider the reaction 2NO2(g)→N2O4(g) Calculate ΔG at 298 K if the partial pressures of NO2 and...
Consider the reaction 2NO2(g)→N2O4(g) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.37 atm and 1.62 atm , respectively
For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) If a reaction vessel...
For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) If a reaction vessel initially contains an N2O4 concentration of 4.50×10−2 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?
The reaction 2NO(g) + O2(g) 2NO2(g) is second order in NO and first order in O2....
The reaction 2NO(g) + O2(g) 2NO2(g) is second order in NO and first order in O2. When [NO] = 0.2 M and [O2] = 3.4 M, the observed rate of disappearance of NO is 0.00001265 M/s. A) What is the value of the rate constant? B) What are the units of the rate constant? - M0 s-1 - M-3 s-1 - s-1 - M3 s - M-1 - M1 s1 - M-1 s-1 - M-1 s-2 - M-2 s-1 -...
1) Initial concentration of reactant A in a 2nd-order reaction aA ----> Products is 0.880 M....
1) Initial concentration of reactant A in a 2nd-order reaction aA ----> Products is 0.880 M. In 30 min, the concentration of A decreases to 40.0% of its initial value. Determine the rate constant of this reaction 2) For the reaction N2O4(g) = 2NO2(g), the equilibirum constant at definite temperature Kc = 3.5 x 10^-4. If the initial concentration of N2O4 is 0.200M, what will be the concentration of NO2 at equilibrium?
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction. 2 NO2(g) → 2 NO(g)...
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction. 2 NO2(g) → 2 NO(g) + O2(g) The rate constant at 273 K is 2.3 ✕ 10-12 L/mol · s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 4.0 atm to 2.4 atm at 451 K? Assume ideal gas behavior.
Consider the reaction: 1/2 N2(g) + O2(g)<<<----->>>NO2(g) Write the equilibrium constant for this reaction in terms...
Consider the reaction: 1/2 N2(g) + O2(g)<<<----->>>NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and bbelow: a.) N2O4(g) <-------> 2NO2(g) Ka b.) N2(g) + 2 O2(g) <------> N2O4(g) Kb K =
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT