Ametal salt with the formula MCI2 crystallizes from water to form a solid with the composition MCl, - 6H,0. The equilbrium vapor pressure of water above this solid at 298 K is 16.8 mbarPart AWhat is the value of A,G for the reactionMCla - 6 H20(s) = MCla(s) + 6 Hạ0(a)when the pressure of water vapour is 16.8 ubur ?Express your answer as an integer with the appropriate units.HAA,G= ValueUnitsSubmitPravinus Answers Requast AnsWarPart BWhat is the value of A,G"?Express your answer with the appropriate units.IH HẢA,G° =ValueUnitsSubmitPrevious Answers Request Answer

The reaction is – MCl2.6H2O s ⇔MCl2s +6H2Og

Ametal sak vih he femal MCI, aystalies fom water to fom a soid with fhe compotion MCl, - GiH,0 The rquilbrium vaper pressure of water above this soid at 230 Kis 158 mbar. • Part A What is the value of AGler the reaction MC - 6 H;0(») = MClg(•) + ©H;OG) nhen the pressure of water vapour is 16.8 alur ? Express your answer as an integer with the appropriate units. A,G= Value Units Previeen Ann Reest Anser Submit • Part B What is the value of A;G°? Express your answer with the appropriate units. HÁ ? A;G° = Value Units Submit Previous Answers Request Answer

Ametal sak vih he femal MCI, aystalies fom water to fom a soid with fhe compotion MCl, - GiH,0 The rquilbrium vaper pressure of water above this soid at 230 Kis 158 mbar. • Part A What is the value of AGler the reaction MC - 6 H;0(») = MClg(•) + ©H;OG) nhen the pressure of water vapour is 16.8 alur ? Express your answer as an integer with the appropriate units. A,G= Value Units Previeen Ann Reest Anser Submit • Part B What is the value of A;G°? Express your answer with the appropriate units. HÁ ? A;G° = Value Units Submit Previous Answers Request Answer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Suppose a certain small bird has a mass of 30 g. What is the minimum mass of glucose that it must consume to fly to a branch 10 m above the ground? The change in Gibbs energy that accompanies the oxidation of 1.0 mol C6H12O6(s) to carbon dioxide and water vapour at 25 °C is -2828 kJ.
Consider a body of water in equilibrium with solid calcium sulfate, CaSo4, for which Ksp= 3.0 x 10^-5 at 25 degrees C. Calculate the solubility, in g/L, of calcium sulfate in water assuming that other reactions are negligible. *
The decomposition vapor pressure of NH4Cl at 421°C was 618 kPa and increased to 1215 kPa at 459°C.NH4Cl(k) NH3(g) + HCl(g)(a) the equilibrium constant,(b) the standard reaction Gibbs energy,(c) standard enthalpy,(d) Calculate the standard decomposition entropy, all at 421°C.Note that steam behaves like an ideal gas and that ΔH° and ΔS° are independent of temperature in the given range.Assume it is.
The decomposition of a generic diatomic element in its standard state is represented by the equation 1/2 X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.34 kJ·mol−1 at 2000. K and−50.82 kJ·mol−1 at 30003000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, ΔGf=4.34 kJ·mol−1. What is K at that temperature?
The standard Gibbs energy of formation of PH3 (g) is 13.4 kJ/mol at 298 K. What is the corresponding reaction Gibbs energy when the partial pressures of the H2 and PH3(treated as perfect gases) are 1.0 bar and 0.60 bar, respectively? What is the spontaneous direction of the reaction in this case?
The decomposition of a generic diatomic element in its standard state is represented by the equation 1/2 X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.58 kJ·mol−1 at 2000 K and −52.64 kJ·mol−1 at 3000. K. Determine the value of the thermodynamic equilibrium constant, ?K, at each temperature. At 2000 K, ΔGf=5.58 kJ·mol−1. What is ? at that temperature? At 3000 K, Δ?f=−52.64 kJ·mol−1. What is K at that temperature?
Coiled coils are protein domains that lead to the formation of multimers (dimers,trimers, tetramers, etc.). They are found in a wide range of proteins. Here we willconsider the trimerization reaction. We may write the chemical equilibrium as3 M(aq) ⇄ T(aq)where M and T represent, respectively, the monomer and trimer species. Given that∆rG0 = −25.00 kJ mol−1 at 37 0C (with the standard state the normal one for reactionsin solution, namely c0 = 1.0 mol dm−3):A) What is the equilibrium constant for the formation of the trimer at 37 0C? B) Suppose that in a particular experiment at 37.00 0C the initial concentrations ofthe monomer if [M]0 = 2.00×10−2 µM and the initial concentration of the trimeris also [T]0 = 2.00 × 10−2 µM. What is ∆rG for the formation of the trimer atthe specified temperature? C) For the conditions given in part (B) will trimers spontaneously convert to monomers?Give a very short justification of your answer. D) Suppose that ∆rH0 and ∆rS0 are independent of the…
The solubility constant Ksp for barium oxalate is 1.6 x10-6 . Determine the standard Gibbs free energy delta G degree for the dissolution of BaC2O4 at 25 degrees
1) Determine the solubility product constant (Ksp) of borax, a slightly soluble sodium salt, in water at two different temperatures and evaluate the enthalpy, entropy and Gibbs free energy change for dissolving borax in water. Materials and reagents: Borax (Na2B4O5(OH)4· 10H2O) Na2CO3 0.1 M HCl solution Bromocresol green indicator Bromothymol blue indicator 500 ml Erlenmeyer flasks (10 per student) Beakers (2 per student) Magnetic stirrer and bar (1 per student) Distilled water Ice-water bath Thermometer (1 per student) 50 ml burette (1 per student) Procedure: Preparation of the Borax-Borate Equilibrium Mixtures: These solutions will be prepared beforehand. Take about 60 mL of each solution. Make sure each student performs at least one titration. To two separate 500mL Erlenmeyer flasks containing magnetic stirring bars add about 20g of borax and 400mL of distilled water. Designate one flask as the room temperature system and one as the ice-water system. Stir the room…
Ethanoic acid (acetic acid) was evaporated in container of volume 21.45 cm3 at 437 K and at an external pressure of 101.9 kPa, and the container was then sealed. The mass of acid present in the sealed container was 0.0519 g. The experiment was repeated with the same container but at 471 K, and it was found that 0.0380 g of the acid was present. Calculate the equilibrium constant for the dimerization of the acid in the vapour, and the standard enthalpy of the dimerization reaction.
Consider the following reaction: NH4Cl--->NH3(g)+HCl(g). The vapor pressure after dissasociation of a certain amount of NH4Cl is 608 kPa at 427 Celsius, but rises to 1115 kPa at 459 Celsius. Calclate Keq, deltarGstandard, and deltarHstandard, all at 427 Celsius. Assume that the vapor is an idela gas and that the enthalpy is indepednet of temperature in the range given.
The difference in chemical potential of a particular substance between two regions of a system is +7.1 kJ mol−1. By how much does the Gibbs energy change when 0.10 mmol of that substance is transferred from one region to the other?