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Chapter 5 Solutions
EBK 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_forwardAmmonia reacts with water in liquid ammonia solution according to the equation: NH3(g) + H2O ⇌ NH4+ + OH− The change in enthalpy for this reaction is 21 kJ/mol, and ΔS° = −303 J/(mol·K). What is the equilibrium constant for the reaction at the boiling point of liquid ammonia (−31°C)?arrow_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
- 15. 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_forwardThe 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_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
- Write 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_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
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