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Chemical Kinetics

Kinetics - Reaction

Please see the attached file. 4. The following data were measured for the reaction: BF3 (g) + NH3 (g) -> F3 BNH3 (g) experiment [BF3] (M) [NH¬3] (M) Initial rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 a. what is the rate

Orders of Reaction

The rate of the following reaction in aqueous solution is monitored by measuring the number of moles of Hg2Cl2 that precipitate per liter per minute. The data obtained are listed in the table. 2HgCl2 + (C2O4^2-) ----> (2Cl^-) + 2CO2 (g) + Hg2Cl2 (s) Experiment [HgCl2],M ([C2O4]^2-),M Initial rate,m

The half-life for the first-order decomposition of sulfuryl chloride

The half-life for the first-order decomposition of sulfuryl chloride at 320 degrees Celsius is 8.75 h. SO2Cl2 (g) -----> SO2 (g) + Cl2 (g) (a) What is the value of the rate constant k, in s^-1? (b) What is the pressure of sulfuryl chloride 2.52 h after the start of the reaction, if its initial pres

Reaction Rates

The rate of the following reaction in aqueous solution is monitored by measuring the rate of formation of (I3^-). The data obtained is listed in the table. (S2O8^2-) + (3I^-) ----> (2SO4^2-) + (I3^-) Experiment ([S2O8]^2-), M ([I]^-),M Initial rate, M s^1- 1 0


The smog constituent peroxyacetyl nitrate (PAN) dissociates into peroxyacetyl radicals and NO2 (g) in a first-order reaction with a half-life of 32 min. If the initial concentration of PAN in an air sample is 5.9 x 10^14 molecules/L, what will be the concentration 1.05 h later? (in molecules/L)

Reaction Rates

In the first-order decomposition of dinitrogen pentoxide at 335 K, assume we start with a 2.50 g sample of N2O5 at 335 K and have 1.50 g remaining after 109 s. N2O5 (g) -----> 2NO2 + 1/2 O2 (a) What is the value of the rate constant k? (in s^-1) (b) What is the half-life of the reaction? (in s) (c) What mass of N2O5 w

Reactions and Rate Equations

(a) From the rate constant k1 = 3.66 x 10^-3 s^-1 compute the instantaneous rate (r1) of the first-order decomposition of 2.30 M H2O2 (aq). (in mol L^-1 s^-1) (b) From the rate constant k2 = 1.24 x 10^-2 L mol^-1 s^-1 compute the instantaneous rate (r2) of the second-order decomposition of 2.04 M C8H9O3 (l). (in mol L^-1

Mole Fraction

What is the mole fraction of urea, CO(NH2)2, in a solution prepared by dissolving 31.0 g CO(NH2)2 in 118 mL of water at 20 degrees Celsius (d= 0.998 g/mL)?

Determining weight %; ppm by mass; and solubility of alum?

Problem Statement: Chemical XYZ is added to a substrate at a defined rate of 1.17% of the dry weight of the substrate; paper makers alum (Al2(SO4)3-14H2O) is added to the substrate at a rate of 45% of the Chemical XYZ rate; the dry weight of the substrate is given as 1460 lbs/1000 ft2 The molecular weight of the alum is g

Rate Equation for Atmospheric Oxidation of S(IV) to S(VI)

A) Calculate the liquid phase / gas phase ratio for SO2, HNO3, HCl and H2O2 in a cloud droplet (L= 10-6) and determine which phase dominates. b) Explain why the atmospheric rate of formation of S(VI) in the aqueous phase is given by (Please see attachment for atmospheric rate of formation) where k is the liquid-phase rate

Steady State Pollution Concentration from Box Model for City

1) Consider an urban area (100 km^2) with a temperature profile that decreases linearly with height between 30 degrees C at the surface, and 24 degrees C at 500 m. At 500 m, the temperature increases with height to 30 degrees C at 1000 m. What is the mixing height for this situation? Using a box model for the city, calculate

Five physical chemistry questions.

5) Ozone decomposes to oxygen according to the balance chemical equation below: 2O3 ---> 3O2 If the rate of disappearance of the ozone is -7.2E-4 M/s, what is the rate of formation of oxygen? 6) If 100kJ of heat is added to 54.0 g of water at 100°C, what is the final state of the water? MW H2O = 17.9 g/mole 7) How many

Vmax, Km: Calculation of Kinetic Constants, first order

The initial velocity of an enzyme catalyzed reaction was measured at a serious of different initial substrate concentrations in the table. Find Km (sometimes called Ks)(the half velocity constant) and ...there is moreshow problemThe initial velocity of an enzyme catalyzed reaction was measured at a serious of different initial s

Reaction data for the reaction of Pt(bipy)Cl2 with ethylenediamine was analyzed to obtain a rate constant and reaction orders. Graphs were produced and calculations performed.

In SXR205 Activity B, the kinetics of the reaction between the square-planar platinum complex dichloro-(2,2'-bipyridine) platinum (II) (Pt(bipy)Cl2) and 1,2-diaminoethane (en) were investigated. In a different study of this reaction, the data in Table 1 were obtained manually using a spectrometer set at a fixed wavelength of 274

Chemical Formulas for the ionic compounds

See attached file for full problem description. 1. what is the chemical formula for the following ternary compounds given their constituent ions a. lead(IV) sulfate b. stannous chlorite c. cobalt(II) hydroxide d. mercurous phosphate 2. Provide the formula for each of the following binary ionic compounds a. curprous su

Reaction Order

If the overall reaction is the sum of the order of the reagents, and: Zero order = changing concentration of the reactant does not affect the reaction rate. First order = doubling the concentration of any reactant doubles the reaction rate Second order = doubling the concentration of any reactant quadruples the reaction

Fractional Distillation

Explain why packed and spinning band fractional distillation columns are more efficient at separating two liquids having close boiling points than are unpacked columns.

Moles and Volume

A solution of an unknown agent was titrated with 30.0 mL of a 0.100 M chromate solution, which causes the chromate to be reduced to Cr3. If instead of chromate, a 0.100 M permanganate solution had been used that resulted in the formation of Mn2+, what volume of permanganate solution would be required?

Reaction Rate

I AM TRYING TO FIND THE ACTIVATION ENERGY My slope is (-4295.5) My R is the Gas constant=8.314 How do I utilize the Arrhenius formula to get the Activation energy? Also, how do I calculate th slope of log K compared to 1/Temp?

Rates of Reactions - Simple

1. Explain why the rate of a simple chemical reaction such as: NO(g) + 1O2(g) → NO2(g) is likely to be most rapid at the beginning of the reaction. 2. If you wish to dissolve a lump of sugar in water, give three ways you could increase the rate at which the sugar dissolves? Explain why each procedure is effective.

Methanol Production Process

Methanol production process is operated at temperatures of 25 - 30 degrees & a pressure of 50 - 100 atmospheres, in the presence of a copper based catalyst. Comment on whether these operating conditions (250 - 300 degrees & 50-100 atmospheres) are consistent with the aims of achieving a high equilibrium yield of methanol and a h


1.) At 40 degrees Celsius CH2O2(aq) will decompose according to the following reaction: 2H2O2(aq) ----- 2H2O(l) + O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2

Copper percipitate

Trying to figure out how much copper should precipitate from a reaction between .55g of zinc and 92.4mL of copper sulfate. What formula would I use?

Rate Constant and Order of Reactions

I need help understanding how to determine orders of reaction: 1. For a first order reaction w/rate constant of .35 sec-1, the percent starting material remaining after 25 sec is: 2. Rate data for the reaction 2 NOBr (g)->; 2 NO (g) + Br2 (g) follows: [NOBr] Rate (mol L-1 s-1) .0450 1.62 x 10-3 .0310 7.69 x 10-4

Activation energy and reaction rates

The rearrangement of cyclopropane to propene has been studied at various temperatures. Experimental values for the rate constants are as follows (please see the attachment for the table). a) Determine the best value for the activation energy for this reaction b) Predict the best value for k at 500 K Make sure to acco

Reaction Rate, Temperature & the Arrhenius Equation

The rate of a particular reaction triples when the temprature is increased from 25C to 35C. Calculate the activation energy for this reaction. Also i just need to clearify the concept of Arrhenius Equation. What happened to Rate Constant(k) and the rate of reaction if: a. there is a decrease in temperature b. an increase in

Second order rate law calculations

Second order rate law: 1/[N02]=0.775L/(mol*s)* 645s+1/.0030mol/L= 8.3*10^2L/mol Please provide step-by-step mathematical operation of the above.