The rate constant for a reaction is 0.447the activation energy for this reaction?Lmol sLat 315 K and 405.8 at 385 K. Using the Arrhenius equation, what ismol s-In k₂ — In kıEa = -R(+)-(+)•Recall that R is the ideal gas constant (8.314(8.314Jmol K.).• Report your answer with three significant figures.Provide your answer below:J/mol

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Answered: The rate constant for a reaction is…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 56QRT

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In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q were expressed in units of pressure. We also can use units of mol/L for the quantities in Q, specifical.ly for aqueous reactions. With this in mind, consider the reaction HF(aq)H+(aq)+F-(aq) for which Ka = 7.2 104 at 25C. Calculate G for the reaction under the following conditions at 25C. a. [HF] = [H+] = [F] = 1.0 M b. [HF] = 0.98 M, [H+] = [F] = 2.7 102M c. [HF] = [H+] = [F] = 1.0 105 M d. [HF] = [F] = 0.27 M, [H+] = 7.2 104M e. [HF] = 0.52 M, [F] = 0.67 M, [H+] = 1.0 103M Based on the calculated G values, in what direction will the reaction shift to reach equilibrium for each of the five sets of conditions?
7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
Calculate G for the dissolution of both sodium chloride and silver chloride using data from Appendix E. Explain how the values you obtain relate to the solubility rules for these substances.
In Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If this reaction is so product-favored, why can large piles of yellow sulfur exist in our environment (as they do in Louisiana and Texas)?
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.
Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH3 CO2H+ C2H; OH = CH3 C02C,H; + H2O К — 2.2 Acetic acid Ethanol Ethyl acetate For the following mixtures, will the concentration of H2 O increase, decrease, or remain the same as equilibrium is established? а. [CH3CO-С2H:] — 0.22 М, [Н,0] — 0.10 М, [CH3 CO2H] — 0.010 М, [С, Нs Он] — 0.010 м decrease increase O remain the same b. [CH3 CO2 C2H3] 3D 0.22 М, [Н2о) —D 0.0020 М, [СH; CO2H] — 0.0020 М, [С2H5 ОН — 0.10 м decrease X increase O remain the same c. [CH3 CO2C2H3] 3D 0.88 М, [Н20] - 0.12 М, [СH3СО2Н 3D 0.044 М, [С Hs ОН — 6.0м decrease O remain the same increase d. [CH; CO2C2H;] 3D 4.4 М, [Н20] %3D 4.4 М, [СН3СОН — 0.88 м, [С, H; ОН] — 10.0м increase O remain the same decrease e. What must the concentration of water be for a mixture with [CH3CO2 C2H5] = 1.0 M, [CH3CO2H] = 0.10 M, and [C2H5 OH] = 6.0 M to be at equilibrium? Concentration = 0.09 X M
40. For the reaction S,(g) = 2 S(g), log1, K, = – 16.735 at 1000°K, while AH° = 102,600 + 2.47 T – 0.444 × 10-3 T² Find the extent to which S,(g) will be dissociated into atoms at a temperature of 4000°K and 1 atm pressure.
3a) please see attached
The equilibrium constant for the reaction of decomposition of AB3 (AB3(g)= A(g)+ 3B (g)) is %3D [A][B]³ K = [AB3] where [A], [B] and [AB3] are the concentrations of A, B and AB3 respectively. Use the properties of logarithms to obtain the -log[B] as a function of logK, log[A] and log[AB3].
Consider the reaction: NO(g) + C₂H₂(g) → HCN(g) + CO(g) + H(g), is The Arrhenius expression for the reaction is k(T) = 8.97 x 10-¹2 cm³ molec-¹ s¹ exp{-218 kJ mol-¹/RT} over the temperature range 1100 - 1500 K. Using transition state theory, calculate AH* and AS* for this reaction at 1300 K.

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