Constants I Periodic TablePart AFor the following reaction studied in the gas phase (Fridgen, T. D., et al. J.Phys. Chem. A 2005, 109, 7519):Ci-+ C3H7CN → C1C3H7+ CN-Is the overall reaction exothermic or endothermic?Match the words in the left column to the appropriate blanks in the sentence on the right.the following potential energy surface was derived:[Cl–C;H;-CN]¯Reset HelpClC;H,+ CNexothermicThe overall reaction isbecauseat a higher energyendothermicthanthe products arethe reactants areCl +C;H¬CNthe transition state is[CIC;H,-CN]SubmitRequest Answer[Cl–C;H;CN]Reaction progressPart BThe mechanism for the reaction, based on the potential energy diagram,There are six activation energies, one associated with each of the rate constants in the mechanism. Two of the elementary steps are barrierless, in that they have activationcan be written as:energies equalling zero. Which of the six activation energies, Eal, Ea–1 Ea2 Ea-2 Ea3 Ea-3 are equal to zero?kCi¯+ C3H7 [Cl – C3H7CN]-Check all that apply.k[CIC3H7 – CN]Eal[Cl – C3H7CN]k,Ea-1[CIC3H7 – CN]CIC3H7+ CNEa2Еa-2Ea3Ea-3Energy

A) The overall reaction is endothermic because the products are at a higher energy than the reactant…

Constants I Periodic Table • Part A For the following reaction studied in the gas phase (Fridgen, T. D., et al. J. Phys. Chem. A 2005, 109, 7519): CI+ C3H7CN - CIC3H7 + CN Is the overall reaction exothermic or endothermic? ¯ Match the words in the left column to the appropriate blanks in the sentence on the right. the following potential energy surface was derived: [CI-C,H,-CN] Reset Help CICH,+ CN exothermic The overall reaction is because at a higher energy endothermic than the products are the reactants are CI +C;H;CN the transition state is [CIC;H,-CN] Submit Request Answer CI-C,H,CN] - Reaction progress- • Part B The mechanism for the reaction, based on the potential energy diagram, There are six activation energies, one associated with each of the rate constants in the mechanism. Two of the elementary steps are barrierless, in that they have activation energies equalling zero. Which of the six activation energies, Eal, Ea-1 Ea2 Ea-2 Ea3 Ea-3 are equal to zero? can be written as: CI+ C3H7 (CI – C3H7CN] Check all that apply. O Eal (C1 - C3H7CN] (CIC3H7 - CN]- Ea-1 [CIC3H7 - CN] CIC3H7 + CN Ea2 Ea-2 O Ea3 Ea-3

Constants I Periodic Table • Part A For the following reaction studied in the gas phase (Fridgen, T. D., et al. J. Phys. Chem. A 2005, 109, 7519): CI+ C3H7CN - CIC3H7 + CN Is the overall reaction exothermic or endothermic? ¯ Match the words in the left column to the appropriate blanks in the sentence on the right. the following potential energy surface was derived: [CI-C,H,-CN] Reset Help CICH,+ CN exothermic The overall reaction is because at a higher energy endothermic than the products are the reactants are CI +C;H;CN the transition state is [CIC;H,-CN] Submit Request Answer CI-C,H,CN] - Reaction progress- • Part B The mechanism for the reaction, based on the potential energy diagram, There are six activation energies, one associated with each of the rate constants in the mechanism. Two of the elementary steps are barrierless, in that they have activation energies equalling zero. Which of the six activation energies, Eal, Ea-1 Ea2 Ea-2 Ea3 Ea-3 are equal to zero? can be written as: CI+ C3H7 (CI – C3H7CN] Check all that apply. O Eal (C1 - C3H7CN] (CIC3H7 - CN]- Ea-1 [CIC3H7 - CN] CIC3H7 + CN Ea2 Ea-2 O Ea3 Ea-3

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter21: Rates Of Chemical Reactions, Ii. A Clock Reaction

Section: Chapter Questions

Problem 2ASA

See similar textbooks

Similar questions

The thermal decomposition of potassium chlorate can be used to produce oxygen. 2KClO3 --> 2KCl +3O2 What volume of O2 gas at 298 K and 1.0 atm pressure is produced by the decomposition of 7.50 g of KClO3 (FW=122.6)?
What is the magnitude of teh uncertainity associated with each of the following measurements. a) 317.0? b) 0.0317?
What is ΔSsurr for a reaction at 28.6 °C with ΔHsys = 38.9 kJ mol-1 ? Express your answer in J mol-1 K-1 to at least two significant figures.
A N2 molecule at 20 ⁰C is released at sea level to travel upward. Assuming that the molecule does not collide with other molecules, how far will it travel before coming to rest? Do the same calculation for a He atom. Hint: to calculate the height h, the molecule will travel, equate its kinetic energy with the potential energy it attains at h, which is mgh. Here m is the mass, and g is the gravitational acceleration
The average bond enthalpies of the C—F and C—Cl bondsare 485 kJ/mol and 328 kJ/mol, respectively. (a) What isthe maximum wavelength that a photon can possess andstill have sufficient energy to break the C—F and C—Clbonds, respectively? (b) Given the fact that O2, N2, andO in the upper atmosphere absorb most of the light withwavelengths shorter than 240 nm, would you expect thephotodissociation of C—F bonds to be significant in thelower atmosphere?
Vanadic ion, V3+, forms green salts and is a good reducingagent, being itself changed in neutral solutions to thenearly colorless ion V(OH)4+. Suppose that 15.0 mL of a0.200-M solution of vanadic sulfate, V2(SO4)3, was neededto reduce completely a 0.540-g sample of an unknownsubstance X. If each molecule of X accepted just oneelectron, what is the molecular weight of X? Suppose thateach molecule of X accepted three electrons; what wouldbe the molecular weight of X then?
why would you write 13.90 when only two sig figs were given? Where does the extra "precision" come from?
Use the equations: PV = 2/3 n KE and PV = nRT to derive KE = 3/2 RT
The highest building in Montreal is the ‘1 square building’, with a height of 203m.The atmospheric pressure in the streets of Montreal is P1 = 9.9 x 104Pa.Suppose air density is constant : ρair= 1,2 kg/m3 and g = 9.8 m/s2. Suppose the rooftop temperature to be T = 298K, and the air composition is 100%N2 molecules. The collision cross-section of N2 molecules is 0.43 nm2.*f. Find the collision frequency. Is it in the order of magnitude that you wereexpecting?
For the equation 2K + Cl2------>2KCl. I understand Cl is diatomic , but where does the 2 in front of the K come from.
1) Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2(g) ® SO2(g) + Cl2(g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 liter bulb and the temperature is raised to 375K. (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375K. Note: Please answer both A and B
1) Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2(g) ® SO2(g) + Cl2(g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 liter bulb and the temperature is raised to 375K. (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375K. (c) Give the expression for the equilibrium constant (either Kp or Kc) for the decomposition of SO2Cl2(g) at 375K. Calculate the value of the equilibrium constant you have given, and specify its units. (d) If the temperature were raised to 500K, what effect would this have on the equilibrium constant? Explain briefly. Note: Please answer just C and D. Thank you.