If the plot of ln(Ksp) versus 1/T for a thermodynamic reaction yields a straight line with positive slope and positive y-intercept, what can be said about the spontaneity of the reaction?
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If the plot of ln(Ksp) versus 1/T for a
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- If the plot of ln Ksp versus 1/T for a reaction yields a straight line with positive slope and positive y-intercept, what can be said about the spontaneity of the reaction?Chemistry show all work Calculate the PV work associated with the combustion of ethane (C2H6) at 298 K.The 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?
- Is a Hess' Law calculation a direct determination of a standard heat of reaction? Discuss.Thermodynamics. Prove the relationship. (dP/dT)G = S/Vor the reaction2CO2(g) + 5H2(g)C2H2(g) + 4H2O(g)H° = 46.5 kJ and S° = -125 J/KAt standard conditions, this reaction would be product favored at no temperature. at all temperatures. at relatively high temperatures. at relatively low temperatures
- 18 Estimate the difference between ΔHreaction and ΔUreaction (in kJ/mol) for the reaction: 6Li(s) + N2(g) →2Li3N(s) at 298 K 23 Use standard enthalpies of formation to determine ΔHoreaction for the following reaction: 2N2H4(l) + N2O4(g) →3N2(g) + 4H2O(g)The entropy of reaction at T=198.15K and a pressure of 5 bar.Discuss the effect of temperature on the spontaneity of reactions with the following values for H and S. (a) H =128kJ;S =89.5J/K (b) H =20.4kJ;S =156.3J/K (c) H =127kJ;S =43.2J/K
- THIS PROBLEM HAS TWO PARTS I CONFUSED ON PART 2 I HAVE ALREADY FIGURED OUT PART A BUT I HAVE INCLUDED IT BECAUSE PART B WOULDN'T MAKE SENSE WITHOUT IT. a) For the boiling point of ethanol is 173.1 F. In an experiment the entropy change for the reaction CH3CH2OH(l) yields CH3CH2OH (g) the entropy change was determined to be 120.9 J/mol K. Please estimate the enthalpy if evaporation. ANSWER FOR PART A: -42.5kJ PART B (THE PART I NEED HELP WITH) For the reaction in part A determine the SIGNS of ΔH and the SIGNS and VALUE of ΔG at 100 F. (Note Δ H can be - or +) and ΔG can be (-,0,+)Using acetic acid and the reduction of acetate to acetaldehyde as an example, let’s investigate the difference between the “chemical standard state” (Xo or XƟ) and the “biochemical standard state” (Xo' or X'o). Given the following reaction and associated data at T = 298.15 K. a) Calculate ΔfGo' for CH3COOH(aq) and CH3COO-(aq). b) Even though by definition, ΔfGƟ (H+(aq)) = 0 and ΔfGo' (H+(aq)) = 0, these are different physical quantities. What precisely does each represent? c) Calculate the pKa of acetic acid. Gibbs free energy of formation, in units of kjmol-1, at T=298.15K ΔfGƟ ΔfGo' CH3COOH(aq) -396.5 CH3COO-(aq) -369.3 H+(aq) 0 0The standard entropies at 298 K for certain group 4A elementsare: C(s, diamond) = 2.43 J/mol-K, Si1s2 = 18.81 J/mol-K, Ge1s2 = 31.09 J/mol-K, and Sn1s2 = 51.818 J/mol-K. All but Sn have the same (diamond) structure. Howdo you account for the trend in the S° values?