(a) The heat evolved upon dissolution of atmospheric ozone into water is determined to be +5 kcal/mol at 298 K. Given that ozone has a Henry’s constant of 9.4 × 10−3 mol/L/atm at 298 K, determine its Henry’s constant at 273 K. Note that the definition of Henry’s constant is for the process air to water. (b) If the atmospheric ozone concentration in a polluted air is 100 ppbv, what is the concentration in equilibrium with a body of water in that region at 298 K? Note that you need to assume no losses of ozone other than absorption into water

(a) The heat evolved upon dissolution of atmospheric ozone into water is determined to be +5 kcal/mol at 298 K. Given that ozone has a Henry’s constant of 9.4 × 10−3 mol/L/atm at 298 K, determine its Henry’s constant at 273 K. Note that the definition of Henry’s constant is for the process air to water. (b) If the atmospheric ozone concentration in a polluted air is 100 ppbv, what is the concentration in equilibrium with a body of water in that region at 298 K? Note that you need to assume no losses of ozone other than absorption into water

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 91QRT: Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium...

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Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Select the reaction for which K, = Kc. 2 Na,0,(s) + 2 CO,(g) =2 Na,CO3(s) + 0,(g) 2 KCIO3 (s) = 2 KCI(s) + 30,(g) 2 H,S(g) + SO,(g)= 3 S(s) + 2 H,O(g) Br, (g) + Cl,(g) 2 BRCI(g)
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?
C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalyst
2 Zn*2 (aq) +Fe*2 (ag) + 6 CN (ag) = Zn2Fe(CN)6 (5) [znz Fe (CN),] A certain equilibrium reaction has K = 2.8 x 10-13 at 25 °C. What is the change in Gibbs Free Energy (kJ/mole) under these conditions?
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium? ....... J/mol The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 68 oC is Keq = 401,568. (b) What is the standard reaction Gibbs energy of this reaction?.....J/mol
(a) Adsorption of a gas on surface of solid is generally accompanied by a decrease in entropy, still it is a spontaneous process. Explain.(b) Some substances can act both as colloids ’ and crystalloids. Explain.(c) What will be the charge on Agl colloidal particles when it is prepared by adding small amount of AgNO3 solution to KI solution in water ? What is responsible for the development of this charge ?
b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079
› Calculate the value of the equilibrium constant, Kỵ, for the reaction Q(g) + X(g) — 2M(g) + N(g) given that Kc = M(g) — Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.48 Kc2 Kc3 = 0.587 = = 13.6
Calculate the value of the equilibrium constant, Kc , for the reaction Q(g)+X(g)↽−−⇀2M(g)+N(g) given that M(g)↽−−⇀Z(g) Kc1=3.92 6R(g)↽−−⇀2N(g)+4Z(g) Kc2=0.494 3X(g)+3Q(g)↽−−⇀9R(g) Kc3=14.0
Calculate the percentage change in Kx for the reaction CH3OH(g) + NOCl(g) ⇋ HCl(g) + CH3NO2(g) when the total pressure is increased from 1.0 bar to 2.0 bar at constant temperature.
Calculate the value of the equilibrium constant, Ke , for the reaction Q(g)+X(g) = 2 M(g)+N(g) given that M(g) = Z(g) 6 R(g) = 2 N(g) + 4 Z(g) Kel 3.65 Kc2 = 0.420 3 X(g) + 3 Q(g) 9R(g) Kc3 13.4 K.