The rate constant for the reaction is 0.59 x 106 cm mo 5 x 103 mol L? 1+1+Ar→12+Ar s at 293 K. What is the half-life of I if [l 210 mol L1 and [Ar]-
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
In a first-order reaction at 300 K, the half-life is 2.50 x 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 350 K? 4.78 s-1 2.79 x 10-5 s-1 6.38 x 1016 s-1 7.47 x 10-8 s-1 1.03 x 10-2 s-1
55) The rate constant for a first-order reaction is 0.54 s-1. What is the half-life of this reaction if the initial concentration is 0.33 M? 56) The rate constant for a zero-order reaction is 0.54 s-1. What is the half-life of this reaction if the initial concentration is 0.33 M? 57) The reaction that occurs in a Breathalyzer, a device used to determine the alcohol level in a person's bloodstream, is given below. If the rate of appearance of Cr2(SO4)3...
1-The rate constant of a chemical reaction was measured at several temperature values and a plot of ln k (on the y-axis) was plotted against 1/T (on the x-axis, temperature was measured in Kelvin). If the slope of the plot was -9.21 x 103 K and the y-intercept was 13.0, what is the activation energy (EA) of the reaction in kJ mol-1? 2-In an enzyme-catalyzed reaction, the rate of the reaction depends on which of the following at very low...
1)The rate law of a reaction is rate =k[X]³. The units of the rate constant areL mol-1 s-1mol² L-2 s-1mol L-1S-2L² mol-2 s-1mol L-1S-12)Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate =k[X]³[Y]²[Z]⁰The rate of reaction will increase by a factor of136803)What data should be plotted to show that experimental concentration data fits a first-order reaction?1 / [reactant] vs. time[reactant] vs. timeln (k) vs. Ealn (k) vs. 1 / Tln [...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k k and not on the reactant concentration. It is expressed as t1/2=0.693k t 1 / 2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t1/2=1k[A]0. A certain first-order reaction (A→products A → p r o d u c t s ) has a rate constant of 9.30×10−3...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as t 1/2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t 1/2 = 1 k[A ] 0 Part A A certain first-order reaction ( A→products ) has a rate constant of 9.90×10−3 s −1 at 45 ∘...
9. Given the initial rate data below, what is the rate law for the following reaction? 2CIO2(aq)2OH (aq) > CIO3 (aq) CIO2 (aq) H20 [ОН 1о (mol L) Initial rate [CIO2lo (mol L) (mol L s 0.100 0.100 0.23 0.200 0.050 0.46 0.200 0.100 0.92 b) rate k[CIO2][OH] e) rate k[CIO2]3 c) rate [CIO2]OH 12 a) rate k[CIO2][OH ] k[CIO2] [OH] = d) rate = 13I to drop to 95% of its initial value? The 10. How long does it...
Suppose the surface-catalyzed hydrogenation reaction of an unsaturated hydrocarbon has a rate constant of 0.673 M'min. The reaction is observed to follow zero-order kinetics. If the initial concentration of the hydrocarbon is 5.40 M, what is the half-life of the reaction in seconds? *Please report 3 significant figures. Numbers only, no unit. No scientific notation. QUESTION 14 The rate law of a reaction is ratek[X][Y). The units of the rate constant are L mol-1-1 L2 mol-2-1 mol L-1.1 mol2 L-2-1...