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
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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...
1. For the decomposition of NOBr given by 2NOBr(g)⇌ 2NO(s)+Br2(g) If the equilibrium concentrations of these...
1. For the decomposition of NOBr given by 2NOBr(g)⇌ 2NO(s)+Br2(g) If the equilibrium concentrations of these three chemicals are 0.46 M , 0.10 M, and 0.30M calculate a) the value of Kc b) the value of Kp c) the value of Kc if all given concentrations are doubled 2. For the reaction; H2(g) + Br2 ⇌ 2HBr (g) If I start with 0.10 M Hydrogen and 0.20 M bromine what are the equilibrium concentrations of each if Kc = 62.5?...
2NOBr(g) - 2NO (g) + Br2 (g) Reached equilibrium when the concentrations were: [NOBr] = 0.10...
2NOBr(g) - 2NO (g) + Br2 (g) Reached equilibrium when the concentrations were: [NOBr] = 0.10 M, [NO] = 0.010 M, and [Br2] = 0.0050 M . What Is the equilibrium constant for this reaction
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
2NOBr(g) ⇆ 2NO(g) + Br2(g) If nitrosyl bromide, NOBr, is 25.48 percent dissociated at 25°C and...
2NOBr(g) ⇆ 2NO(g) + Br2(g) If nitrosyl bromide, NOBr, is 25.48 percent dissociated at 25°C and the total pressure is 0.325 atm, calculate KP and Kc for the dissociation at this temperature.
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....
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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