- Ch.1 - Matter, Measurement & Problem Solving106
- Ch.2 - Atoms & Elements97
- Ch.3 - Molecules, Compounds & Chemical Equations134
- Ch.4 - Chemical Quantities & Aqueous Reactions115
- Ch.5 - Gases98
- Ch.6 - Thermochemistry84
- Ch.7 - Quantum-Mechanical Model of the Atom49
- Ch.8 - Periodic Properties of the Elements81
- Ch.9 - Chemical Bonding I: The Lewis Model79
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory78
- Ch.11 - Liquids, Solids & Intermolecular Forces41
- Ch.12 - Solids and Modern Material35
- Ch.13 - Solutions66
- Ch.14 - Chemical Kinetics83
- Ch.15 - Chemical Equilibrium52
- Ch.16 - Acids and Bases107
- Ch.17 - Aqueous Ionic Equilibrium130
- Ch.18 - Free Energy and Thermodynamics74
- Ch.19 - Electrochemistry87
- Ch.20 - Radioactivity and Nuclear Chemistry50
- Ch.21 - Organic Chemistry143
Chapter 18, Problem 89a
Consider this reaction occurring at 298 K: N2O(g) + NO2(g) ⇌ 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating ΔG°rxn.
Video transcript
Determine the sign of ΔSsys for each process. a. water boiling
Determine the sign of ΔSsys for each process. b. water freezing
Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to form nitric acid. One of the possible reactions is shown here. Calculate ΔG° and K p for this reaction at 25 °C and comment on the spontaneity of the reaction. 3 NO2(g) + H2O(l )→ 2 HNO3(aq) + NO(g)
Consider this reaction occurring at 298 K: N2O( g) + NO2( g) ⇌ 3 NO( g) b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous?
Consider this reaction occurring at 298 K: N2O(g) + NO2(g) ⇌ 3 NO(g) c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?
Consider this reaction occurring at 298 K: BaCO3(s) ⇌ BaO(s) + CO2( g) a. Show that the reaction is not spontaneous under standard conditions by calculating ΔGrxn ° .