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- In a study of the formation of HI from its elements, H2(g) + 12(g) == 2HI(g) equal amounts of H2 and 12 were placed in a container, which was then sealed and heated. (a) On one set of axes, sketch concentration vs. time curves for H and HI, and explain how Q changes as a function of time. (b) Is the value of Q different if [12] is plotted instead of [H2]?For the reaction of the ammonium ion with nitrous acid, the net reaction is NH4*(aq) + HNO2(aq) → N2(g) + 2H2O() + H*(aq) If the initial concentration of nitrous acid is 1.00 M and, after 28.8 s has elapsed, the concentration of nitrous acid has fallen to 0.82 M, what is the average rate of the reaction over this time interval? 0.0063 M/s 0.028 M/s -0.0063 M/s -0.028 M/s O 0.063 M/sIf the initial concentration of XY is 0.225 mol·L−1, how long will it take for the concentration to decrease to 6.95 × 10−2 mol·L−1 ?. Half life (t1/2)= 1336s or 1.336x103
- A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1: NgÐ — Nz + 0 N₂O + O N₂ + O2 step 2: (a) Identify the molecularity of each step in the mechanism. step 1 8 step 2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. 8 (c) Identify any intemediates and/or catalysts in this mechanism. Catalyst: Enter formula. If none, leave box blank: Intermediate: Enter formula. If none, leave box blank: The following mechanism has been proposed for the gas phase reaction of nitrogen monoxide with bromine. step 1: NO + Br₂ → NOBr₂ NOBr₂ + NO 2 NOBr step 2: (a) Identify the molecularity of each step in the mechanism. step 1 step 2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (c) Identify any intermediates and/or catalysts in this mechanism. Catalyst: Enter formula. If none, leave box blank: Intermediate:…4 Consider the following hypothetical reaction: A(E) + 2B(€) + 4C(g) = 4D(aq) A sophisticated artificial-intelligence model has predicted the following reaction rates for the appearance of D, for varying reagent concentrations, at room temperature: [A]. (mol dm) 8,40 x 105 (B). (mol dm) 1.25 x 10 [C). (mol dm) 1.37 x 104 Rate (mol dm min') 2.58 x 1015 Experiment 8.40 х 105 1.25 х 101 6.85 x 10 1.29 х 10-15 2.50 x 10 2.50 x 10 6.85 x 10 6.85 x 10 3 8.40 x 10 1.29 x 10 15 4 1.68 x 104 5.16 х 10-15 4.20 x 105 6.25 x 102 6.85 х 105 3.23 х 10-16 4.1 Write down the rate law, indicating the order of each reactant concentration with respect to the reaction rate. (Show all your working and reasoning) 4.2 Calculate the reaction rate constant k, including units.1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2C102(aq) + 2OH(aq) → ClO₂ (aq) + CIO; (aq) + H₂O(!) A kinetic study of this reaction under a certain set of conditions yielded the data below. Exp [CIO₂] (M) [OH-] (M) A[CIO₂]/At (M/s). 0.100 1 5.75 x 10-2 2 0.100 3 0.0500 0.0500 0.100 0.100 0.10 0.25 2.30 x 10-¹ 1.15 x 10-¹ a. What is the rate law? b. What is rate constant, k? c. fill in the missing cell in the table.
- 8 Reactions between certain organic (alkyl) halides and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane). (CH3)3CBr(aq) + H2O(1) →(CH3)3COH(aq) + H*(aq) + Br "(ag) k[(CH3)3CB1]. The accepted mechanism for the The experimental rate law is rate = %3D reaction is shown below. (1) (CH3)3C-Br(aq) →(CH3)3C*(aq) + Br "(aq) [slow] (2) (CH3)3C*(aq) + H2O(1) →(CH3)3C-OH2*(aq) [fast] (3) (CH3)3C-OH2*(aq) →H*(aq) + (CH3)3C-OH(aq) [fast] a) Why doesn't H2O appear in the rate law? b) Write rate laws for the elementary steps. c) What intermediates appear in the mechanism? d) Show that the mechanism is consistent with the experimental rate law. ed to the of consumption of N5. The rate at which a chemical is depleted from a solution is proportional to the concentration of the chemical in the solution. (a) Determine the difference equation (not differential equation) that represents the concentration of the chem- ical C(t) as a function of time. (b) Derive the differential equation that represents the concentration of the chemical C(t) as a function of time. (c) Solve the differential equation with C(0) = Co to obtain C(t).(a) Explain the meaning of the sentence:“The velocity laws of reactions are empirical” (b) It can be determined that the velocity law of a generic reaction A +B→Pév = k[A]x[B]y. Plot on a graph the variation of [A] and [P] with time, and explain why v= d[P]/dt = -d[A]/dt. (c) Explain the meaning of the terms k, x and y, in the velocity law, presented in item b: (d) Explain what it means in practice for a velocity law to be of zero order. Plot ,A as a function of t, for the zero-order reaction A→Products. (e) Explain what elementary reactions are and how they can be classified.
- The iodate ion is reduced by sulfite according to the followingreaction:IO3-(aq) + 3 SO32-(aq) -----> I-(aq) + 3 SO42-(aq)The rate of this reaction is found to be first order in IO3-,first order in SO32-, and first order in H+.(a) Write the rate law for the reaction.(b) By what factor will the rate of the reaction change ifthe pH is lowered from 5.00 to 3.50? Does the reactionproceed more quickly or more slowly at the lower pH?(c) Explain how the reaction can be pH-dependent even thoughH+ does not appear in the overall reaction.The enzyme urease is widely used for determining urea concentration in blood. The Michaelis constant for urease at room temperature is 2.0 mM and k2 = 2.5 × 10^3 s^-1 at pH = 7.5. Based on the kinetic experiment, when 4.76 mM urease was used, the initial rate of the reaction was determined to be 8.1 M/sec. What is the concentration in unit of mM of urea in blood? Please keep your answer to two decimal place. Please convert all concentration unit to mM in calculation. The answer is 4.26 (I would need help getting this answer)Identify the oxidizing agent in the chemical reaction 5Fe+2(aq) + MnO4-(aq) + 8H+(aq) 5Fe+3 + Mn+2(aq) + 4H2O(l) The answer is ……………………………… Calculate the total number of atoms in 500 Ml OF 0.200 M KNO3 solution. The answer is ……………………………… Mg has three stable isotopes. Given a sample of Mg with the following masses and percent abundances: 24Mg: 23.9850 amu, 58.42% 25Mg: 24.9858 amu, 15.22% 26Mg: 25.9826 amu, 26.36% The average atomic mass (in amu) is …………………… What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M The answer is ………………………