4) A reaction is performed to study the reaction of nitrogen dioxide with carbon monoxide: NO2...
4)
A reaction is performed to study the reaction of nitrogen dioxide with carbon monoxide:
- NO2 + CO ---> NO + CO2
The following reaction rate data was obtained in four separate
experiments.
| Experiment | [NO2]0, M | [CO]0, M | Initial Rate, Ms-1 |
| 1 | 1.54 | 0.435 | 1.33 |
| 2 | 3.08 | 0.435 | 5.31 |
| 3 | 1.54 | 0.870 | 1.33 |
| 4 | 3.08 | 0.870 | 5.31 |
What is the rate law for the reaction and what is the numerical
value of k?
Complete the rate law in the box below.
Remember that an exponent of '1' is not shown and concentrations
taken to the zero power do not appear.
| Rate = |
k = ___
M-1s-1.
Homework Answers
Rate law for given reaction.
As concentration of NO2 double the rate of reaction becomes four time
Rate = k[NO2]2
Form exp 1
K = 1.33/(1.54)2
K =0.561
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4)
A reaction is performed to study the reaction of
nitrogen dioxide with carbon monoxide:
NO2...
A reaction is performed to study the oxidation of nitrogen monoxide by oxygen at 25 °C:...
A reaction is performed to study the oxidation of
nitrogen monoxide by oxygen at 25 °C:
2 NO + O22
NO2
The following reaction rate data was obtained in four separate
experiments.
Experiment
[NO]0, M
[O2]0, M
Initial Rate, M/s
1
9.10×10-3
4.40×10-3
3.11×10-3
2
1.82×10-2
4.40×10-3
1.24×10-2
3
9.10×10-3
8.80×10-3
6.22×10-3
4
1.82×10-2
8.80×10-3
2.49×10-2
What is the rate law for the reaction and what is the numerical
value of k?
Complete the rate law in the box below....
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Nitrogen dioxide, NO2 decomposes into nitrogen monoxide (NO) and oxygen gas O2 , according to the...
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carbon monoxide reacts with nitrogen dioxide to produce carbon dioxide and nitric oxide as given by...
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The reaction between nitric oxide (nitrogen monoxide) and oxygen gives nitrogen dioxide according to the stoichiometric equation. 2 NO(g) 02(g)2 NO2(g) 1. Write the rate law expected if the reaction was found to occur in a single step The reaction is observed to be complex with the following mechanism is proposed: 2 NO N202 N202 2 NO N202 +02 → 2NO2 k2 kı k. -1 2. Use the steady state approximation to obtain the expression for the formation of NO2....
A) B) The following initial rate data are for the reaction of nitrogen dioxide with fluorine:...
A)
B)
The following initial rate data are for the reaction of nitrogen dioxide with fluorine: 2 NO2 + F2 → 2 NO2F Experiment [F2), M [NO2], M 3.19 3.19 1.20 2.40 IllII Initial Rate, Ms-1 4.40x10-4 8.80x10-4 8.80x10-4 1.76x10-3 6.38 1.20 6.38 Complete the rate law for this reaction in the box below. Use the form k[A][B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1...
A reaction is performed to study the oxidation of
nitrogen monoxide by oxygen at 25 °C:
2 NO + O22
NO2
The following reaction rate data was obtained in four separate
experiments.
Experiment
[NO]0, M
[O2]0, M
Initial Rate, M/s
1
9.10×10-3
4.40×10-3
3.11×10-3
2
1.82×10-2
4.40×10-3
1.24×10-2
3
9.10×10-3
8.80×10-3
6.22×10-3
4
1.82×10-2
8.80×10-3
2.49×10-2
What is the rate law for the reaction and what is the numerical
value of k?
Complete the rate law in the box below....
The following initial rate data are for the reaction of nitrogen dioxide with carbon monoxide NO2 + CO >NO + CO2 [NO2lo, M 0.552 0.552 1.10 1.10 [COlo, M 0.461 0.922 0.461 0.922 Initial Rate, Ms1 0.193 0.193 0.768 0.768 Experiment 3 4 Complete the rate law for this reaction in the box below Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1...
Nitrogen monoxide (NO) reacts with oxygen (O2) to form nitrogen dioxide (NO2): NO(g) + O2(g) → NO2(g) Initial rates for the reaction of nitrogen monoxide (NO) and oxygen (02) were measured at 25°C starting with various concentrations of NO and O2. The following data were collected: Exp. [NO]. (A) [02]. (A) d[NO]/dt (M/s) 0.020 0.010 -0.056 0.020 0.020 -0.112 3 0 .020 0.040 -0.224 0.040 0.020 -0.448 5 0.010 0.020 -0.028 4 What is the numerical value of the rate...
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B)
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