Question

For the reaction 2NO2 (g) -> 2NO (g) + O2 (g), data for rate constants was...

For the reaction 2NO2 (g) -> 2NO (g) + O2 (g), data for rate constants was obtained at the following temperatures.

L1 L2 L3 L4
Temperature, K k, M-1 s-1 1/T, K-1 Ln k
330 0.77
354 1.8
378 4.1
383 4.7

What happens to the rate constant as temperature increases?

Find the A and Ea graphically using linear regression.

Find Ea using the two-data point approach with the data at 330 K and 383 K. Why is there a slight difference?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Arhenius equation is K=Ko*e(-Ea/RT), Ko= Frequency factor and Ea= activation energy and R= gas constant =8.314 J/mole.K

takin ln, lnK= lnKo-Ea/RT, so a plot of lnK vs 1/T gives straight line whose slope is -Ea/R and intercept is lnK

the plot of lnK vs 1/T is generated and shown below.

from the plot of best fit, -Ea/R= slope =-4344.2, Ea= 4344.2*8.314 J/mole =36118 J/mole= 36.12 Kj/mole

for two different temperatrues, T1 and T2, Arhenius equation is

ln(K2/K1)= (Ea/R)*(1/T1-1/T2)

given T1= 330K and T2= 383K, K2= 4.7 and K1= 0.77

ln(4.7/0.77)= (Ea/8.314)*(1/330-1/383)

Ea= 35864.76 J/mole= 35.864 KJ/mole

the activation energy calculated accounting for all the points is based on the best fit of the plot of lnK vs 1/T.

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
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures...
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ and ΔS∘ do not change too much within the give temperature range.) a. 298 K b. 721 K c. 853 K
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures...
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ and ΔS∘ do not change too much within the give temperature range.)    1. 298 2. 722 3. 860
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures...
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ and ΔS∘ do not change too much within the give temperature range.) A) 298K B) 733K C) 853K
1)calculate the equilibrium constants at 25∘C for each reaction. Part A 2NO(g)+O2(g)⇌2NO2(g) Express your answer using...
1)calculate the equilibrium constants at 25∘C for each reaction. Part A 2NO(g)+O2(g)⇌2NO2(g) Express your answer using two significant figures. Part B N2(g)+O2(g)⇌2NO(g) Express your answer using two significant figures. 2) Calculate the change in Gibbs free energy for each of the following sets of ΔHrxn, ΔSrxn, and T. Part A ΔH∘rxn=+ 85 kJ , ΔSrxn=+ 155 J/K , T= 298 K Express your answer as an integer. Part B ΔH∘rxn=+ 85 kJ , ΔSrxn=+ 155 J/K , T= 753 K...
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
The following data were collected for the rate of disappearance of NO in the reaction 2NO(g)+O2(g)→2NO2(g):...
The following data were collected for the rate of disappearance of NO in the reaction 2NO(g)+O2(g)→2NO2(g): Experiment [NO](M) [O2](M) Initial Rate (M/s) 1 0.0126 0.0125 1.41×10−2 2 0.0252 0.0250 1.13×10−1 3 0.0252 0.0125 5.64×10−2 What is the rate of disappearance of NO when [NO]= 6.70×10−2 M and [O2]= 1.98×10−2 M ? What is the rate of disappearance of O2 at the concentrations given in part (d)?
For the reaction 2NO(g) + O2(g) → 2NO2(g), ∆H° = -113.1 kJ/mol and ∆S° = -145.3...
For the reaction 2NO(g) + O2(g) → 2NO2(g), ∆H° = -113.1 kJ/mol and ∆S° = -145.3 J/K·mol. Under which temperature conditions would the reaction be spontaneous?
34. Consider the reaction 2NO(g) + O2(g) ⇆ 2NO2(g) At a certain temperature, an equilibrium mixture...
34. Consider the reaction 2NO(g) + O2(g) ⇆ 2NO2(g) At a certain temperature, an equilibrium mixture consists of 0.0230 mole O2, 0.0470 mole NO, and 0.919 mole of NO2. Calculate KP for the reaction, given that the total pressure is 0.200 atm. KP =
For the reaction 2NO(g) + O2(g) ⇄ 2NO2(g) ∆rxnG0 = −72.6 kJ/mol At 600 K, if...
For the reaction 2NO(g) + O2(g) ⇄ 2NO2(g) ∆rxnG0 = −72.6 kJ/mol At 600 K, if a reaction vessel initial has partial pressures of pNO2(g) = 107 Pa, pNO(g) = 2 Pa, and pO2(g) = 2Pa, in which direction will the reaction occur, forwards or backwards?
the following data were obtained for the reaction, 2NO2(g)-->2NO (g) + O2. Times   (NO2) 0   0.8333...
the following data were obtained for the reaction, 2NO2(g)-->2NO (g) + O2. Times   (NO2) 0   0.8333 20   0.4167 40   0.2778 60   0.2083 c) what is the reaction order with respect to NO2? explain D) write the rate law for this equation
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT