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a possible mechanism for the overall reaction is found below:Br2(g)+2NO(g)--->2NOBr(g). step 1: (fast) NO(g)+Br2(g)-->&<---NOBr(g) determine the...
The rate equation for the reaction 2NO(g) + Br_2(g) rightgarrow 2NOBr(g) was determined experimentally to be: Rate = k[NO]^2 [Br_2] 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) + Br_2 (g) rightarrow 2NOBr (g) (ii)NO (g) + Br_2 rightwardsharpoonoverleftwardsharpoon NOBr_2 (g) NOBr_2 (g) + NO (g) rightarrow 2NOBr (g) (iii) Br_2 rightwardsharpoonoverleftwardsharpoon Br +...
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...
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....
For the following two-step mechanism: Step 1: NO (g) + NO (g) --K1--> N2O2 (g) (fast, equilibrium) <------- Step 2: N2O2 (g) + Br2 (g) ------> 2 NOBr (g) (slow) (a) Write the equation for the overall reaction. (b) Write the raw law for the overall reaction.
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?
The equilibrium constant for the reaction: 2NO(g) + Br2(g) <----> 2NOBr(g) is Kc = 1.3x10^-2 at 1,000 Ka.) At this temperature, does the equilibrium favor the product or reactants?b.) Calculate Kc for 2NOBr <----> 2NO + Br2c.) Calculate Kc for NOBr <----> NO + 1/2Br2
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
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...
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?
A student ran the following reaction in the laboratory at 254 K: 2NO(g) + Br2(g) ⇌ 2NOBr(g) When she introduced 0.185 moles of NO(g) and 0.130 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.152 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =