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CM-UY 1004 Lecture Notes - Lecture 8: Reaction Rate, Fokker E.Ii, Haber Process

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25 Aug 2016

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Temperature and rate, rates generally increase as the temperature rises, the collision model b. i. The greater the number of collisions/s the greater the reaction rate b. ii. 1. As reactant concentration increases, the number of collisions increases, leaning to an increase in reaction rate b. iii. Svante arrhenius suggests that molecules must possess a certain minimum amount of energy to react d. ii. This energy comes from the kinetic energies of the colliding molecules d. iii. d. iv. At higher temperature a greater fraction of the molecules have kinetic energy greater than ea, which leads to a greater rate of reaction d. v. d. vi. The fraction of molecules that have an energy equal to or greater than the activation energy is given by: d. vi. 1. Order in which the bonds are broken and formed, and the changes in relative positive of the atoms in the course of the reaction: elementary reactions b. i. Elementary reactions are reactions that occur in a single event or step b. ii.

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In the collision model it is assumed that reactions occur as a result of collisions between molecules with the correct kinetic energy and orientation. The minimum energy required for a reaction to occur when molecules collide is called the activation energy, E_a. The number of collisions that are favorably oriented for a reaction is described by the frequency factor, A. The Arrhenius equation relates both of these factors to the rate constant, k. k = A middot e^-E_a/(R middot T) where R = 8.314 J/(mol middot K) and T is the temperature in kelvins. Based on the activation energies and frequency factors, rank the following reactions from fastest to slowest reaction rate, assuming they are all at the same temperature. Rank from fastest to slowest reaction rate. To rank items as equivalent, overlap them. Fraction of molecules The exponential term in the Arrhenius equation is equal to the fraction of molecules, f, with kinetic energy greater than or equal to the activation energy: f = e^-E_a/(R middot T) Most scientific calculators have an e^x function as the second function of the LN button. Part B A certain reaction with an activation energy of 145 kJ/mol was run at 495 K and again at 515 K. What is the ratio of f at the higher temperature to f at the lower temperature? Express your answer numerically using one significant figure. In the collision model it is assumed that reactions occur as a result of collisions between molecules with the correct kinetic energy and orientation. The minimum energy required for a reaction to occur when molecules collide is called the activation energy, E_a. The number of collisions that are favorably oriented for a reaction is described by the frequency factor, A. The Arrhenius equation relates both of these factors to the rate constant, k: k = A middot e^-E_a/(R middot T) where R = 8.314 J/(mol middot K) and T is the temperature in kelvins. Part A Based on the activation energies and frequency factors, rank the following reactions from fastest to slowest reaction rate, assuming they are all at the same temperature. Rank from fastest to slowest reaction rate. To rank items as equivalent, overlap them. Fraction of molecules The exponential term in the Arrhenius equation is equal to the fraction of molecules, f, with kinetic energy greater than or equal to the activation energy: f = e^E_a/(R middot T) Most scientific calculators have an e^x function as the second function of the LN button. Part B A certain reaction with an activation energy of 145 kJ/mol was run at 495 K and again at 515 K. What is the ratio of f at the higher temperature to f at the lower temperature? Express your answer numerically using one significant figure. In the collision model it is assumed that reactions occur as a result of collisions between molecules with the correct kinetic energy and orientation. The minimum energy required for a reaction to occur when molecules collide is called the activation energy, Ea. The number of collisions that are favorably oriented for a reaction is described by the frequency factor, A. The Arrhenius equation relates both of these factors to the rate constant, k: k = A middot e^-E_a/(R middot T) where R = 8.314 J/(mol middot K) and T is the temperature in kelvins. Fraction of molecules The exponential term in the Arrhenius equation is equal to the fraction of molecules, f, with kinetic energy greater than or equal to the activation energy: f = e^-E_a/(R middot T) Most scientific calculators have an e^x function as the second function of the LN button. Part B A certain reaction with an activation energy of 14 kJ/mol was run at 495 K and again at 515 K. What is the ratio of f at the higher temperature to f at the lower temperature? Express your answer numerically using one significant figure.

Chemical reactions occur when molecules or atoms collide, the bondsbetween atoms are broken, and new bonds are formed. Breaking thebonds of the reactants requires energy; bond formation releasesenergy. Which of the following statements regarding energy changesduring a reaction are true?
(A)The activation energy (Ea) of the forward reaction is thedifference between the energy of the products and the energy of thetransition state.
(B)If the heat of reaction, ?H, is positive, the energy of theproducts is lower than the energy of the reactants, and thereaction is endothermic.
(C)When the activation energy is low, the reaction rate isslow.
(D)Two or more atoms must collide, with proper orientation, withenergy greater than or equal to the activation energy for areaction to occur.
(E)Increasing the concentration of reactants increases the numberof collisions, and the reaction goes faster.
(F)The energy of a collision between atoms or molecules must begreater than the activation energy (Ea) for bonds to bebroken.
(G)Decreasing the temperature decreases the kinetic energy of thereactants, and the reaction goes more slowly.