![The rate equation for the reaction 2NO(g) + Br2(g) → 2NOBr(g) was determined experimentally to be: (b) Rate = k[NO]2[Br] Five possible mechanisms have been proposed (i) - (v) Determine the rate equation for each mechanism below and then decide with reasons, (based on the information given) which mechanism is the most likely. (i) 2NO(g) + Br2(g) →2NOBr (g) NO (g)+ Br2 NOBr2(g)+NO(g) (ii) NOBT2(g) -) 2NOBr (g) (iii) Br2= Br + Br + NO (g) → NOBr (g) Br + NO (g) → NOBr (g) NO (g) + Br2(g) Br (iv) → NBr2(g) → 2NOBr (g) fast slow NBr2 (g) + O2 (g) →N2O2 (g) slow fast (v) 2NO (g) N2O2(g) + Br2(g) → 2NOBr (g)](http://img.homeworklib.com/questions/c689bd10-3875-11eb-ad60-e1e042e02c67.png?x-oss-process=image/resize,w_560)
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The rate equation for the reaction 2NO(g) + Br_2(g) rightgarrow 2NOBr(g) was determined experimentally to be:...
In the endothermic reaction 2NOBr(g) = 2NO(g) + Br2(g) at equilibrium, which of the following changes...
In the endothermic reaction 2NOBr(g) = 2NO(g) + Br2(g) at equilibrium, which of the following changes will result in an increase in the partial pressure of NOBr? 1. decreasing the partial pressure of Br2 II. increasing the size of the reaction vessel III. lowering the overall temperature of the reaction IV. adding a catalyst V. adding He(g) O A I and II I and II O B lland III O c IV and V IV and V III and V...
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was...
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was determined experimentally to be Rate kINO] [02]. Two mechanisms have been proposed for this reaction: Mechanism A Mechanism B 2NO N202 NO O2 NO3 NO3 + NO → 2NO2 N202 O22NO2 (i) Determine the rate equation for the formation of NO2 by both mechanisms. (i) Under what conditions will both of these mechanisms fit the experimental data? (i) Suggest one reason why either mechanism...
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
for the reaction 2NOBr(g)---- 2NO(g)+Br2(g) the rate of the reaction -2.3 mol NOBr/L/h when the initial...
for the reaction 2NOBr(g)---- 2NO(g)+Br2(g) the rate
of the reaction -2.3 mol NOBr/L/h when the initial NOBr
concentration was 6.2 mol NoBr/L. what is the rate constant of the
reaction.
Please help:)
52. For the reachon ZNO Brly) - 2Noig) + Brela) the rate of the reaction was -23 mol NoBrilh when the inihol NOBY Coventration was 2 mol NOBYL Wat is the rate constant of the reaction?
select all of the mechanisms that are plausible for a given reaction and it's experimentally determined...
select all of the mechanisms that are plausible for a given
reaction and it's experimentally determined the rate law.
10.00 points Select all of the mechanisms that are plausible for the given reaction and its experimentally determined rate law. Overall Reaction: 2NO + CI, + 2NOCI Experimentally Determined Rate Law: rate = k[NO][CI] Step 1: NOCI, + NOCI, (slow) Step 2: NOCI, NQ -- 2NÓCI (fast) Step 1: CI, -+ 2Cl (slow) Step 2: 2NO+2CI2NOCI (fast) Step 1: NOCI, NOCI...
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
The following reaction has an equilbrium constant Kc =3.07e-4 at 24oC. 2NOBr(g) <---> 2NO(g) + Br2(g)...
The following reaction has an equilbrium constant Kc =3.07e-4 at 24oC. 2NOBr(g) <---> 2NO(g) + Br2(g) Decide whether the reaction mixture is at equilibrium, given the conditions below, or if the reaction will go left or right to achieve equilibrium. Type left, right or equilibrium. [NOBr] = 0.103 M [NO] = 0.0134 M [Br2] = 0.0181 M
The square in the reaction equation is an equilibrium sign. Consider the following reaction: 2NOBr(g) 2NO(g)...
The square in the reaction equation is an equilibrium
sign.
Consider the following reaction: 2NOBr(g) 2NO(g) + Br2(g) If 0.485 moles of NOBr(g), 0.623 moles of NO, and 0.470 moles of Br2 are at equilibrium in a 14.9 L container at 494 K, the value of the equilibrium constant, Kc, is The equilibrium constant, K. , for the following reaction is 7.00x10- at 673 K. NHI(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.01...
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...
In the endothermic reaction 2NOBr(g) = 2NO(g) + Br2(g) at equilibrium, which of the following changes will result in an increase in the partial pressure of NOBr? 1. decreasing the partial pressure of Br2 II. increasing the size of the reaction vessel III. lowering the overall temperature of the reaction IV. adding a catalyst V. adding He(g) O A I and II I and II O B lland III O c IV and V IV and V III and V...
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was determined experimentally to be Rate kINO] [02]. Two mechanisms have been proposed for this reaction: Mechanism A Mechanism B 2NO N202 NO O2 NO3 NO3 + NO → 2NO2 N202 O22NO2 (i) Determine the rate equation for the formation of NO2 by both mechanisms. (i) Under what conditions will both of these mechanisms fit the experimental data? (i) Suggest one reason why either mechanism...
for the reaction 2NOBr(g)---- 2NO(g)+Br2(g) the rate
of the reaction -2.3 mol NOBr/L/h when the initial NOBr
concentration was 6.2 mol NoBr/L. what is the rate constant of the
reaction.
Please help:)
52. For the reachon ZNO Brly) - 2Noig) + Brela) the rate of the reaction was -23 mol NoBrilh when the inihol NOBY Coventration was 2 mol NOBYL Wat is the rate constant of the reaction?
select all of the mechanisms that are plausible for a given
reaction and it's experimentally determined the rate law.
10.00 points Select all of the mechanisms that are plausible for the given reaction and its experimentally determined rate law. Overall Reaction: 2NO + CI, + 2NOCI Experimentally Determined Rate Law: rate = k[NO][CI] Step 1: NOCI, + NOCI, (slow) Step 2: NOCI, NQ -- 2NÓCI (fast) Step 1: CI, -+ 2Cl (slow) Step 2: 2NO+2CI2NOCI (fast) Step 1: NOCI, NOCI...
The square in the reaction equation is an equilibrium
sign.
Consider the following reaction: 2NOBr(g) 2NO(g) + Br2(g) If 0.485 moles of NOBr(g), 0.623 moles of NO, and 0.470 moles of Br2 are at equilibrium in a 14.9 L container at 494 K, the value of the equilibrium constant, Kc, is The equilibrium constant, K. , for the following reaction is 7.00x10- at 673 K. NHI(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.01...
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