Find the overall reaction order and the order of the individual reactants of each reaction.1. NO +0.2(g) 3(g)-NO. + O3(g)2. 2NO+2H₂ -N + 2H₂O(g)(g)2(g)3. C₂H6(⁹)4. H₂(g) + Br₂(g) →2HBr (g)25. C₂H₂¹2(g)→2CH3(g)(g)2(g)rate = k[NO₂][0₂]ratek[NO]²[H₂]100. adiin eigen 8 bns Aratek[C₂H₂] brs x etnegograInTenoo st61 eri axrate =_k[H₂][Br₂] artemoidbinte= k[C₂H₂1]muerunoitsupe nevig enMrate- C₂H4(9) + HI(g) arts roirlw of atnanoque erli==1919

order of the reaction is the sum of the exponents of all the reactants in the rate expression.

Find the overall reaction order and the order of the individual reactants of each reaction. 1. NO +0. 2(g) 3(g) -NO. + O 3(g) 2. 2NO+2H₂ -N + 2H₂O(g) (g) 2(g) ¹2(g) 3. C₂H6(g) →2CH3(g) 4. H₂(g) + Br₂(g) →2HBr (g) 5. C₂H₂ (g) 2(g) rate rate = k[NO₂][0₂] k[NO]²[H₂] rate - C₂H49) + Hl(9) art rainw of ethanoque eri 4(g) = rate 190 s br rate = onco, adian piger 8 hrs A k[C₂H₂] bns x atnepogre po ontemointblote InTenoo st61 or 2 x = _k[H₂][Br₂] = k[C₂H₂1] mue or noitsupe nevig en

Find the overall reaction order and the order of the individual reactants of each reaction. 1. NO +0. 2(g) 3(g) -NO. + O 3(g) 2. 2NO+2H₂ -N + 2H₂O(g) (g) 2(g) ¹2(g) 3. C₂H6(g) →2CH3(g) 4. H₂(g) + Br₂(g) →2HBr (g) 5. C₂H₂ (g) 2(g) rate rate = k[NO₂][0₂] k[NO]²[H₂] rate - C₂H49) + Hl(9) art rainw of ethanoque eri 4(g) = rate 190 s br rate = onco, adian piger 8 hrs A k[C₂H₂] bns x atnepogre po ontemointblote InTenoo st61 or 2 x = _k[H₂][Br₂] = k[C₂H₂1] mue or noitsupe nevig en

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 28QRT

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Similar questions

Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Nitrosyl bromide, NOBr, is formed from NO and Br2: 2 NO(g) + Br2(g) 2 NOBr(g) Experiments show that this reaction is second-order in NO and first-order in Br2. (a) Write the rate equation for the reaction. (b) How does the initial reaction rate change if the concentration of Br2 is changed from 0.0022 mol/L to 0.0066 mol/L? (c) What is the change in the initial rate if the concentration of NO is changed from 0.0024 mol/L to 0.0012 mol/L?
Based on the kinetic theory of matter, what would the action of a catalyst do to a reaction that is the reverse of some reaction that we say is catalyzed?
. Account for the increase in reaction rate brought about by a catalyst.
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
Candle wax is a mixture of hydrocarbons. In the reaction of oxygen with candle w ax in Figure 11.2, the rate of consumption of oxygen decreased with time after the flask was covered, and eventually' the flame went out. From the perspective of the kinetic-molecular theory, describe what is happening in the flask. FIGURE 11.2 When a candle burns in a closed container, the flame will diminish and eventually go out. As the amount of oxygen present decreases, the rate of combustion will also decrease. Eventually, the rate of combustion is no longer sufficient to sustain the flame even though there is still some oxygen present in the vessel.
Nitrogen dioxide reacts with carbon monoxide by the overall equation NO2(g)+CO(g)NO(g)+CO2(g) At a particular temperature, the reaction is second order in NO2 and zero order in CO. The rate constant is 0.515 L/(mol s). How much heat energy evolves per second initially from 3.50 L of reaction mixture containing 0.0275 M NO2? See Appendix C for data. Assume the enthalpy change is constant with temperature.

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