For a reaction with multiple reactants (Rate=k[A]m[B]n)(Rate=k[A]m[B]n), how is the overall order of the reaction defined?
For a reaction with multiple reactants , how is the overall order of the reaction defined?
[A]m[B]n[A]m[B]n |
[A]m[A]m |
nn |
mm |
m+nm+n |
[B]n[B]n |
m−nm−n |
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For a reaction with multiple reactants (Rate=k[A]m[B]n)(Rate=k[A]m[B]n), how is the overall order of the reaction defined?...
A)What is the overall order of reaction for a reaction that obeys the rate law rate k[A]²[B]³b) c)
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For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between Aand B, aA+bB⇌cC+dD The dependence of the reaction...
If the rate law for a reaction is rate = k[A]2[B] a. What is the overall order of the reaction? b. If the concentration of A is doubled and the concentration of B is tripled, how will this affect the rate of the reaction? c. How will doubling the concentration of B while holding A constant affect the value of k (assuming that temperature remains constant)?
what is the overall reaction order ? LAU B: KINE 0505 Studying the Rate of the of the Reaction of Potassium Permanganate and Oxalic A Table II Calculated initial concentrations, mol/L Determination Humber H.CO. Average clapsed Pinte, .2+28 sec Ranction rate, mol/L. 2.52x10 m/s 7.98x10-5 m/s &mofl alisec s KMnO m40.10 10.629 move 0,0108moll 217sec 10.315 mol/L 0.027move 426esec 5,09x10m Order of reaction with respect to (a) H.CO. One Overall reaction order (b) KMnO pere one Calculated rate constant, k,...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. What is the reaction order with respect to B? Also, how do you find the value of the rate constant k for this reaction? Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4
Which of the following rate laws represents a reaction that is second order overall? A. rate = k [A][B]2[C] B. rate = k [A]2[B]2[C]2 C. rate = k [A][B] D. none of these E. rate = k [A]2 [B]
3. A reaction has two reactants A and B. What is the order with respect to each reactant and the overall order of the reaction described by each of the following rate expressions? a) rate = ki[A] b) rate = k2[A][B] A=3 A=1 B=0 B=1 c) rate = k3[A][B] d) rate = ka[B] A=0 B=a B=1 What are the units of the rate constants in Question 3 if the rate is expressed in mol/L*min? a) b) 4. b)
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