If the standard free engery change of the reaction S to P is -50kJ mol-1 (-12 kcal mol-1), the reaction will:  (a) never reach equilibrium  (b) proceed spontaneously from left to right  (c) proceed rapidly because of the large negative standard free energy change  (d) never reach equilibrium because of the large large negative standard free energy change

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15. When a solute is able to go spontaneously into solution: (A) both the enthalpy (AHsoln) and the entropy (ASsoln) of mixing are always positive. (B) both the enthalpy (AHsoln) and the entropy (ASsoln) of mixing are always negative. (C) the enthalpy (AHsoln) is always negative, while the entropy (Scoln) is always positive. (D) the enthalpy (AHsoln) may be positive or negative, but the entropy (ASsoln) is always positive. (E) the enthalpy (AHsoln) is always negative, but the entropy (ASsoln) may be positive or negative.

Consider The Following Reaction: CaCO3(S) + 2HCl(Aq) = CaCl2(Aq) + H2O(L) + CO2(G)  Write down the quation of the equilibrium constant kc for this reaction

A reaction has a standard free-energy change of -13.20 kJ mol-(-3.155 kcal mol-). Calculate the equilibrium constant for the reaction at 25 °C. Keq

The following equilibrium constants have been determined for hydrosulfuric acid at 25°C: H2S(aq) = H*(aq) + HS (aq) K¸' = 9.5 × 10-8 HS (aq) = H*(aq) + S²¯(aq) K¸" = 1.0 × 10-19 es Calculate the equilibrium constant for the following reaction at the same temperature: H,S(aq) = 2H*(aq) + s²¯(aq) K = x 10

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the equilibrium constant (K) is a quantitative measurement of theextent to which a chemical or physical reaction proceeds to completion. If two reactants ofknown initial concentration are mixed and then the concentrations of the products aremeasured once equilibrium has been established, then the equilibrium constant can becalculated using an ICE table.In this experiment you will measure the equilibrium constant for the formation of iron(III)thiocyanate from the iron(III) cation and thiocyanate anion:Fe3+(aq) + SCN-(aq) FeSCN2+(aq)The product, FeSCN2+, is intensely red, which means that its concentration can be measured byusing an ultraviolet-visible (UV-vis) spectrophotometer. So long as a solution is not tooconcentrated, the absorption of light at a particular wavelength by a chemical species isdescribed by Beer’s Law:A = εℓ[X] where A = absorption of light (unitless number)ε = molar absorptivity constant (cm-1 M-1)ℓ = path length (cm)[X] = concentration (M)The path length for our…

1. NO2(g) and N₂O4(g) are in a reaction vessel with partial pressures 0.510 bar and 0.800 bar respectively. A,Gº = -2.80 kJ mol-¹. Is this system at equilibrium at 298 K? (a) Yes (b) No

(a) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. ____The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs. -).____A Gibbs free energy change involves moles of substances whereas an emf involves coulombs of electrons.____A coulomb of particles is more particles than a mole of particles.____Faraday's constant is not used to interconvert a Gibbs free energy change and a reaction emf.____A Gibbs free energy change involves coulombs of substances whereas an emf involves moles of electrons.Calculate the standard Gibbs free energy changes at 25 oC for each of the reactions shown below using the Eo values given. Select whether each of these reactions is nonspontaneous, at equilibrium, or spontaneous under standard conditions. (a) 1 Al3+(aq) + 3 Ag(s)  1 Al(s) + 3 Ag+(aq) Eo = -2.459 V Go =________  kJ/mol ____nonspontaneous…