= ○ KINETICS AND EQUILIBRIUM Drawing the reaction energy diagram of a catalyzed reaction Sketch a qualitative reaction energy diagram for a chemical reaction with and without a catalyst. Assume the uncatalyzed reaction is exothermic. Note: Because the sketches are only qualitative, the energies in them don't have to be exact. They only have to have the right relationship to each other. For example, if one energy is less than another, that fact should be clear in your sketch. energy Uncatalyzed reaction reactants Ea reaction coordinate products energy Catalyzed reaction reactants Ea reaction coordinate 0/3 products

= ○ KINETICS AND EQUILIBRIUM Drawing the reaction energy diagram of a catalyzed reaction Sketch a qualitative reaction energy diagram for a chemical reaction with and without a catalyst. Assume the uncatalyzed reaction is exothermic. Note: Because the sketches are only qualitative, the energies in them don't have to be exact. They only have to have the right relationship to each other. For example, if one energy is less than another, that fact should be clear in your sketch. energy Uncatalyzed reaction reactants Ea reaction coordinate products energy Catalyzed reaction reactants Ea reaction coordinate 0/3 products

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.26E

See similar textbooks

Similar questions

Which sentence best describes the following reaction? 2H2(g)+O2(g)2H2O(l)+heat a. It is an endothermic reaction. b. It is an exothermic double-replacement reaction. c. It is a synthesis reaction that is also exothermic. d. It is a decomposition reaction that is also endothermic.
Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.
Iodide, I–, is a catalyst for the decomposition of hydrogen peroxide to give water and oxygen gas: 2 H2O2 (aq) –––> 2 H2O (aq) + O2 (g); ∆Hrxn = –188 kJ/mol Draw a qualitatively accurate reaction diagram (with energy on the y axis, extent of reaction on x axis) to which shows how the path from reactants to products differs between the catalyzed and uncatalyzed versions of the reaction. Label Eain both of the curves. In a few words, define what is meant by “Ea”.
Chemical reaction rates generally double for a 10-K increase in temperature. How large an increase is that in Fahrenheit? what is the answer? a. 10 deg F b. 5.56 K c. 5.56 deg R d. 18 deg F
Carbon dioxide from the atmosphere “weathers”, or dissolves, limestone, CaCO3 by thereaction.CaCO3 (s) + CO2 (g) + H2O (l) → Ca2+ (aq) + 2 HCO3- (aq)What is DH° for this reaction? DH°f CaCO3 (s) = -1206.9 kJ/mol, DH°f CO2 (g) = -393.5 kJ/mol,DH°f H2O (l) = -285.8 kJ/mol, DH°f Ca2+ (aq) = -542.8 kJ/mol, DH°f HCO3 (aq) = -692.0 kJ/mol
Answer true or false to the following statements about energy diagrams and reactions. Q.) Thermal reactions occur via collisions between molecules, and the more energy in those collisions, the greater the rate of the reactions.
Answer true or false to the following statements about energy diagrams and reactions. Q.) One part of a reaction mechanism would be the understanding of which bonds break and form during a reaction. s
Is the following true or false? Catalysis is the acceleration of reactions and is achieved by making the products lower in energy.
When ethanol (CH3CH2OH) burns in oxygen, carbon dioxide and water are formed. (i) Write the equation which describes this reaction. (ii) Using the data below, calculate the value for ∆Ho for the combustion of ethanol. Hof (CH3CH2OH(l)) = - 277.0 kJmol-1 Hof (CO2(g)) = - 393.7 kJmol-1Hof (H2O(l)) = - 285.9 kJmol-1
Draw two reaction energy profiles, one for an endothermic reaction A and one for an exothermic reaction B. Make the profile for reaction A represent a faster reaction than the profile for reaction B. Label Ea and (+) or (-) DErxn in each profile.
Burning methane with oxygen is a highly exothermic reaction. Yet a mixture of methane and oxygen can be kept indefinitely without any reaction occurring. How is this possible?
The conversion of natural gas, which is mostly methane,into products that contain two or more carbon atoms, suchas ethane (C2H6), is a very important industrial chemicalprocess. In principle, methane can be converted into ethaneand hydrogen: 2 CH4(g)----->C2H6(g) + H2(g) In practice, this reaction is carried out in the presence ofoxygen: 2 CH4(g) + 12O2(g)---->C2H6(g) + H2O(g) (a) Calculate K for these reactionsat 25 °C and 500 °C. (b) Is the difference in ΔG° forthe two reactions due primarily to the enthalpy term (ΔH)or the entropy term 1-TΔS2? (c) Explain how the precedingreactions are an example of driving a nonspontaneousreaction, (d) The reaction of CH4 and O2 to form C2H6 and H2O must be carried out carefully to avoid a competingreaction. What is the most likely competing reaction? Cells use the hydrolysis of adenosine triphosphate (ATP)