A chemist fills a reaction vessel with 0.999 g calcium phosphate (Ca3(PO4)2) solid, 0.689 M calcium (Ca²+) aqueous solution, and 0.245 M phosphate (PO₂³²¯)= aqueous solution at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 3- Ca3(PO4)₂ (s) — 3Ca²+ (aq) +2PO³(aq) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. kJ X S ?

A chemist fills a reaction vessel with 0.999 g calcium phosphate (Ca3(PO4)2) solid, 0.689 M calcium (Ca²+) aqueous solution, and 0.245 M phosphate (PO₂³²¯)= aqueous solution at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 3- Ca3(PO4)₂ (s) — 3Ca²+ (aq) +2PO³(aq) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. kJ X S ?

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).
a Calculate K1, at 25C for phosphoric acid: H3PO4(aq)H+(aq)+H2PO4(aq) b Which thermodynamic factor is the most significant in accounting for the fact that phosphoric acid is a weak acid? Why ?
a Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?
The free energy of the combustion of oxalic acid HC2H3O2 at 25.0 ºC is -246.05 KJ/mol. What is the equlibrium constant Ka at 25ºC?
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data: ΔrH∘ΔrH∘ 182.6kJ mol−1 ΔrS∘ΔrS∘ 24.80J K−1 mol−1 T= 7363 K. Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C∘C:? N2(g)+O2(g)→2NO(g) Express your answer numerically to three significant figures.
Consider the reactionI2(g) + Cl2(g)2ICl(g)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.
For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (a) Aqueous iodide ion is oxidized to I21s2 by Hg2 2+1aq2. (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion. (c) In basic solution, Cr1OH231s2 is oxidized to CrO4 2-1aq2 by ClO-1aq2.
The standard free energy of formation of nitric oxide, NO, at 1000. K (roughly the temperature in an automobile engine during ignition) is 78.5 kJ/mol. Calculate the equilibrium constant for the reactionN2(g) + O2(g) 2NO(g)at 1000. K. a. 0.948 b. 1.57 × 105 c. 7.93 × 10–5 d. 6.29 × 10-9 e. -14.8
The equilibrium constant for a chemical reaction is Kc = 902 at 25°C. What is the standard free energy change, ∆G⁰ for this reaction?
As a result of an experiment following measurements were obtained from a cell: ATP concentration of 0.5 mM, ADP concentration of 0.1 mM, inorganic phosphate (Pi) concentration of 2 mM. Under these conditions calculate the actual free energy (ΔG) of the reaction of hydrolysis of ATP to ADP and Pi. (The standard energy (ΔG°) of ATP = −31 kJ/mol; RT = 2.58 kJ/mol)
1. If Q < K, which way will the reaction proceed and why?
Calculate the free energy change that occurs when a reaction has an enthalpy of −315.2 kJ mol−1 and an entropy change of 224.7 J mol−1 K−1 at 211.3 ∘C. What is the equilibrium constant for this reaction at this temperature? Will that constant increase or decrease as the temperature is increased?

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