2NO(g) + Br2(g) = 2NOBr(g) Experiment [NO-] (M) [Br2] (M) Initial Rate (M s-1) 1 0.10...
2NO(g) + Br2(g) = 2NOBr(g)
| Experiment |
[NO-] (M) |
[Br2] (M) | Initial Rate (M s-1) |
| 1 | 0.10 | 0.20 | 24 |
| 2 | 0.25 | 0.20 | 150 |
| 3 | 0.10 | 0.50 | 60 |
| 4 | 0.35 | 0.50 | 735 |
1.) Determine the rate law equation for the reaction.
2.) What is the overall order of the reaction?
3.) What are the value and the units of the rate constant, k?
4.) Write the expression to show how is the rate of disappearance of bromine, Br2, related to the rate of appearance of nitrosyl bromide, NOBr.
5.) If the rate of disappearance of Br2 is 32 Ms-, what is the rate of appearance of the NOBr.
Homework Answers
Add Answer to:
2NO(g) + Br2(g) = 2NOBr(g)
Experiment
[NO-] (M)
[Br2] (M)
Initial Rate (M s-1)
1
0.10...
Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data...
Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data for the initial rate of appearance of NOBr were obtained: Experiment [NO](M) [Br2](M) Initial Rate of Appearance of NOBr(M/s) 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 What is the rate of disappearance of Br2 when [NO]= 8.1×10−2 M and [Br2]= 0.22 M ? Express your answer using two significant figures.
What is the rate of disappearance of Br2 when [NO]= 8.6×10−2 M and [Br2]= 0.31 M...
What is the rate of disappearance of Br2 when [NO]= 8.6×10−2 M and [Br2]= 0.31 M ? Express your answer using two significant figures. The rate of disappearance of Br2 is half the rate of appearance of NOBr, and the initial problem was: Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data for the initial rate of appearance of NOBr were obtained: Experiment [NO](M) [Br2](M) Initial Rate of Appearance of NOBr(M/s) 1 0.10...
I understand a-c, but not d. The answer is 8.4 M/s but I do not know...
I understand a-c, but not d.
The answer is 8.4 M/s but I do not know how to find it.
Consider the gas-phase reaction between nitric oxide and bromine at 273 °C: 2 NO(g) + Brz(8) — 2 NOBr(8). The following data for the initial rate of appearance of NOBr were obtained: Experiment Initial Rate (M/s) 24 2 [NO](M) 0.10 0.25 0.10 0.35 [Br21(M) 0.20 0.20 0.50 0.50 150 60 735 (a) Determine the rate law. (b) Calculate the average...
For the decomposition of nitrosyl bromide at 10 °C 2 NOBr(g)2NO) +Br2(g) the average rate of...
For the decomposition of nitrosyl bromide at 10 °C 2 NOBr(g)2NO) +Br2(g) the average rate of disappearance of NOBr over the time period from t-0s to t 6.48 s is found to be 2.24 102Ms What is the average rate of appearance of Br2 over the same time period? Submit Show Anproach Show Tutor Steps Sulbmit Answer 5 iten attempts remaining
Data for the following reaction are given in the table. 2NO(g) + Br2(g)->2NOBr(g) Experiment [NO],M [Br2],M...
Data for the following reaction are given in the table. 2NO(g) + Br2(g)->2NOBr(g) Experiment [NO],M [Br2],M Initial rate, M/s 1 1.0x10-2 2.0 x10-2 2.4x10-2 2 4.0x10-2 2.0x10-2 0.384 3 1.0x10-2 5.0x10-2 6.0x10-2 What is the rate law for this reaction? b. What is the overall order of the reaction? c. What is the rate constant for this reaction?
Be sure to answer all parts. Consider the equilibrium 2NOBr(g) ⇆ 2NO(g) + Br2(g) If nitrosyl...
Be sure to answer all parts. Consider the equilibrium 2NOBr(g) ⇆ 2NO(g) + Br2(g) If nitrosyl bromide, NOBr, is 21.66 percent dissociated at 25°C and the total pressure is 0.350 atm, calculate KP and Kc for the dissociation at this temperature.
The gas phase reaction of nitric oxide, NO, with bromine, Br2, to produce nitrosyl bromide, NOBr,...
The gas phase reaction of nitric oxide, NO, with bromine, Br2,
to produce nitrosyl bromide, NOBr,
occurs according to the net reaction: A possible reaction
mechanism is:
?1
Step 1: 2 NO ⇌ N2O2
?−1
Step 2: N2O2 + Br2
2NO+Br2 → 2NOBr
2 NOBr
Neither step is faster than the other. What is the order of the
overall reaction, and what is the overall rate constant (expressed
in terms of the individual rate constants for the elementary
steps)?
9....
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s)...
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 59 s.
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s)...
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 89 s. M
Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) ↔ 2NO (g) + Br2 (g)...
Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) ↔ 2NO (g) + Br2 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.21mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium? a) 0.21, 0.21 b) 0.43, 0.43 c) 0.22, 0.42 d) 0.43, 0.22 e) 0.21, 0.11 Please show all work/steps
I understand a-c, but not d.
The answer is 8.4 M/s but I do not know how to find it.
Consider the gas-phase reaction between nitric oxide and bromine at 273 °C: 2 NO(g) + Brz(8) — 2 NOBr(8). The following data for the initial rate of appearance of NOBr were obtained: Experiment Initial Rate (M/s) 24 2 [NO](M) 0.10 0.25 0.10 0.35 [Br21(M) 0.20 0.20 0.50 0.50 150 60 735 (a) Determine the rate law. (b) Calculate the average...
For the decomposition of nitrosyl bromide at 10 °C 2 NOBr(g)2NO) +Br2(g) the average rate of disappearance of NOBr over the time period from t-0s to t 6.48 s is found to be 2.24 102Ms What is the average rate of appearance of Br2 over the same time period? Submit Show Anproach Show Tutor Steps Sulbmit Answer 5 iten attempts remaining
The gas phase reaction of nitric oxide, NO, with bromine, Br2,
to produce nitrosyl bromide, NOBr,
occurs according to the net reaction: A possible reaction
mechanism is:
?1
Step 1: 2 NO ⇌ N2O2
?−1
Step 2: N2O2 + Br2
2NO+Br2 → 2NOBr
2 NOBr
Neither step is faster than the other. What is the order of the
overall reaction, and what is the overall rate constant (expressed
in terms of the individual rate constants for the elementary
steps)?
9....
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