Rank the following compounds in order of INCREASING standard molar entropy. a. H2O2(l), H2O(l), H4O6+2(aq) < < b. FeO(s), Fe2O3(s), FeCl3(s) < <
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(6) Rank the following compounds in order of INCREASING standard molar entropy.
a. H2O2(l), H2O(l), H4O6+2(aq) < <
b. FeO(s), Fe2O3(s), FeCl3(s) < <
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- Estimate reaction enthalpy and predict the sign of reaction entropy included attatchemnt of mecahnism and of original reactionCalculating Thermodynamic Values from an Equilibrium ConstantBackgroundAs discussed in lecture, the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion…If the change of entropy of the surrounding increased by 0.27 KJ/mol.K due t oa reactiob carried out at a 25C tempreture ,which one of these following terms apply to the reaction?cricle all the correct answers. Exergonic endergonic exothermic endothermic
- Calculate the standard reaction entropy (∆????∅) at 298 K for the reaction of carbon dioxide with calcium oxide which proceeds according to the following:CaO(?) + CO2(?) → ?aCO3(?)List the sets of conditions that allow dS, dU, and dH of a process in a system act as a spontaneity condition.When nitric acid is produced industrially, nitrogen monoxide, NO, is first formed at high temperature. Bakefetr reacts NO on cooling further with oxygen to nitrogen dioxide: 2 NO(g) + O2 ⇌ 2 NO2 (g) Table 1: Thermodynamic data at 25°C. Bond ΔfHom Som Cop,m NO(g) 90.25 210.76 29.34 O2(g) 0.00 205.14 29.36 NO2(g) 33.18 240.06 37.20 1) Calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG25o, for reaction (1) at 25°C from the data in Table 1 2) Calculate (with all relevant intermediate calculations) the equilibrium constant K25, for reaction (1) at 25°C. 3) Industrially, however, the reaction does not proceed at 25°C but at 500°C. Therefore, calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG500o, for reaction (1) at 500°C under the assumption that the standard molar heat capacities, Cop, in Table 1 are independent of temperature in the interval [25°C, 500°C]
- 10. The thermodynamic functions for the generic reaction A+B=>C at 25oC are: ΔH=-35.7 kJ/mole; ΔS=-6.95 J/mole*K Calculate ΔG in kJ/mole Group of answer choices 146 -37.7 -35.5 -33.6 2036The Kₛₚ of PbCl₂ is 1.7X10⁻⁵ at 25°C. What is ΔG°? Is it possible to prepare a solution that contains Pb²⁺(aq) andCl(aq), at their standard-state concentrations?What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 342.26 KJ/mole and the ethlapy (ΔH°rxn) is -422.77 J/mol at 33.48 oC?
- The molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1, andthe molar entropy of fusion under the same conditions is ΔfusSm (H2O)=22.0 J K-1 mol-1. Show that(a) ΔfusGm (H2O)=0 at 273.15 K and one atm, (b) ΔfusG,m (H2O) < 0 when the temperature is greaterthan 273.15 K, and (c) ΔfusGm (H2O) > 0 when the temperature is less than 273.15 K.Identify the highest "change in entropy" from guven reactions, also give clear handwritten explanation!What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 301.59 KJ/mole and the ethlapy (ΔH°rxn) is -394.59 J/mol at 27.73 oC? Answers in 2 decimal place , unit is not required.