(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_forwardThe reaction 2CO(g) + O2(g) = 2 CO2(g) is known to be exothermic. According to Le Chatelier's principle, how will this reaction's equilibrium be affected if the reaction temperature is increased? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will increase and the reaction will shift to the right. (D) The equilibrium constant will be unchanged, but the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.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_forward
- The 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_forwardThe 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_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_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_forwardDinitrogen trioxide decomposes to NO and NO2 in an endothermic process (AH = + 40,5 kJ/mol). 4. N2O3 (g) = NO (g) + NO2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. Motivate each prediction fully. (a) Adding more N2O3 (g) (b) Adding more NO2 (g) (c) Decreasing the temperature (d) Increasing the container volumearrow_forward
- The 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_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 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_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning