Question

Consider the following reaction: NO2(g)→NO(g)+1/2O2(g) The following data were collected for the concentration of NO2 as...

Consider the following reaction:

NO2(g)→NO(g)+1/2O2(g)

The following data were collected for the concentration of NO2 as a function of time:

Time (s)(s) [NO2][NO2] (M)(M)
0 1.000
10 0.951
20 0.904
30 0.860
40 0.818
50 0.778
60 0.740
70 0.704
80 0.670
90 0.637
100 0.606

What is the rate of formation of O2 between 50 and 60 s?

Express your answer to two significant figures.

Homework Answers

Answer #1

Rate of the reaction

= - = 2

Or, = -   

Now,

From the table

Rate of disappearance of NO2 between 50 to 60 s

= -

= -

= 0.0074 M/s.

So,

Rate of formation of O2 between 50 and 60 s

= - ×

=   × (0.0074) M/s

= 0.0037 M/s.

= 3.7 × 10-3 M/s ( 2 significant figures) .

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
Consider the reaction: NO2(g) ® NO(g) + ½ O2(g). The data below were collected for the...
Consider the reaction: NO2(g) ® NO(g) + ½ O2(g). The data below were collected for the concentration of NO2 as a function of time. a)Determined the average rate of the reaction between 10 and 20 s. b)Determine the rate of appearance of O2(g) between 10.0 and 20.0 sec Time (s) 0.0 10.0 20.0 30.0 40.0 50.0 [NO2] (M) 1.000 0.951 0.904 0.860 0.818 0.778
The data below show the concentration of N2O5 versus time for the following reaction: N2O5(g)→NO3(g)+NO2(g) Time...
The data below show the concentration of N2O5 versus time for the following reaction: N2O5(g)→NO3(g)+NO2(g) Time (s) [N2O5] (mol L−1) 0 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210 Determine the order of the reaction.
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
1) Consider the reaction shown below. The concentration of NO2 (g) at equilibrium in a container...
1) Consider the reaction shown below. The concentration of NO2 (g) at equilibrium in a container at 25 oC is 0.100 M. Calculate the concentration of N2O4. For reference, Keq = 8.8 at 25 oC. Show your work.
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
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)?
15.28 Consider the following reaction: 2 N2O(g) ? 2 N2(g)+O2(g) A In the first 13.0  s of...
15.28 Consider the following reaction: 2 N2O(g) ? 2 N2(g)+O2(g) A In the first 13.0  s of the reaction, 1.6×10?2  mol of O2 is produced in a reaction vessel with a volume of 0.400  L . What is the average rate of the reaction over this time interval? Express your answer using two significant figures. B. Predict the rate of change in the concentration of N2O over this time interval. In other words, what is ?[N2O]?t? Express your answer using two significant figures.
Time(s) Concentration (M) N2O5 NO2 O2 0 0.0200 0 0 100 0.0169 0.0063 0.0016 200 0.0142...
Time(s) Concentration (M) N2O5 NO2 O2 0 0.0200 0 0 100 0.0169 0.0063 0.0016 200 0.0142 0.0115 0.0029 300 0.0120 0.0160 0.0040 400 0.0101 0.0197 0.0049 500 0.0086 0.0229 0.0057 600 0.0072 0.0256 0.0064 700 0.0061 0.0278 0.0070 Concentrations as a Function of Time at 55 ∘ for the Reaction 2N2O5(g)⟶4NO2(g)+O2(g) A) Use the data in the table to calculate the average rate of decomposition of N2O5 during the time interval 100-200 s B) Use the data in the table...
[I-1] Consider the following data for the gas-phase decomposition of NO2:   2NO(g) ® 2NO(g) + O2(g)...
[I-1] Consider the following data for the gas-phase decomposition of NO2:   2NO(g) ® 2NO(g) + O2(g) Temperature (K) Initial [NO2] (mM) Initial Rate of NO2 Decomposition (mM/hr) 600 1.00 1.94 600 2.00 7.92 700 2.00 187 At 650 K, how many hours will it take for the NO2 concentration to drop from 5.00 mM to 1.00 mM
Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g). If the rate constant for this reaction at 1000 K is...
Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g). If the rate constant for this reaction at 1000 K is 6.0×104M−2s−1, what is the reaction rate when [NO]= 2.90×10−2M and [H2]= 1.80×10−2M? Express your answer using two significant figures. rate =   M/s   SubmitMy AnswersGive Up Part C What is the reaction rate at 1000 K when the concentration of NO is increased to 0.14 M, while the concentration of H2 is 1.80×10−2M? Express your answer using two significant figures.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT