(a) At
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Physical Chemistry
- 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).arrow_forward7:12 Question 15 of 50 Submit For the decomposition of mercury(II) oxide, HgO, to mercury and oxygen: 2HgO(s) → 2Hg(1) + O₂(g) AG = 117.1 kJ What is the standard Gibbs free energy of formation (AGF) of mercury(II) oxide? A) -117.1 kJ/mol B) -58.6 kJ/mol C) +58.6 kJ/mol D) +117.1 kJ/mol Tap here or pull up for additional resources allarrow_forwardThe Δ?vapΔHvap of a certain compound is 19.52 kJ·mol−1 and its ΔSvap is 81.67 J·mol−1·K−1. What is the boiling point of this compound?arrow_forward
- The value of AG° at 241.0 °C for the formation of phosphorous trichloride from its constituent elements, P2(g) + 3 Cl2(g) → 2 PC|3 (g) is kJ/mol. At 25.0 °C for this reaction, AH° is –720.5 kJ/mol, AG° is –642.9 kJ/mol, and AS° is – 263.7 J/K. -584.9 6.28 x 104 1.35 x 105 -856.1 -656.9arrow_forwardThe value of AG° at 241.0 °C for the formation of phosphorous trichloride from its constituent elements, P2(g) + 3 Cl2(g) → 2 PCl3 (g) is kJ/mol. At 25.0 °C for this reaction, AH° is – 720.5 kJ/mol, AG° is –642.9 kJ/mol, and AS° is – 263.7 J/K 6.28 x 104 -656.9 -584.9 -856.1 1.35 x 105arrow_forward15. a) What is Le Chatelier's Principle? Define and explain this concept. b) Support your explanation using an example based on the following reaction, 3H₂(g) + N₂(g) = 2NH3(g).arrow_forward
- The ΔHvap of a certain compound is 46.73 kJ·mol−1 and its ΔSvap is 64.96 J·mol−1·K−1. What is the boiling point of this compound?arrow_forwardWrite the reaction quotient, Q., for each of the following reactions: (a) The first step in nitric acid production, NH3(g) + Oz(g) NO(g) + H20(g) –arrow_forwardThe reaction 3 O2(g) - 2 O3 (g) has ΔH = +285 kJ/mol. Does the equilibrium constant for the reaction increase or decrease when the temperature increases?arrow_forward
- The equilibrium constant for the reaction, 3 H2(g) + N2(g)= 2NH3(g), at a given temperature is 1.4 x 10–7. Calculate the equilibrium concentration of ammonia, if [H2] = 1.2 x 10–2 mol L–1 and [N2] = 3.2 x 10–3 mol L–1.arrow_forwardAt room temperature, the equilibrium constant (Kw) for the self-ionization of water is 1.00 × 10−14. Using this information, calculate the standard free energy change for the aqueous reaction of hydrogen ion with hydroxide ionto produce water. (Hint: The reaction is the reverse of the self-ionization reaction.)arrow_forwardAt −9.01°C the concentration equilibrium constant Kc =9.5 for a certain reaction. Here are some facts about the reaction: Some of the reactants are liquids and solids. The net change in moles of gases is −2 . If the reaction is run at constant pressure, 118./kJmol of heat are absorbed. Using these facts, can you calculate Kc at 15.°C ? Yes. No. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kc at 15.°C will be bigger or smaller than Kc at −9.01°C ? Yes, and Kc will be bigger. Yes, and Kc will be smaller. No.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning