Calculate the standard Gibbs free energy of reaction in each of the following using the standard molar
Question:
Calculate the standard Gibbs free energy of reaction in each of the following using the standard molar entropy values given. Express your answers to 3 significant figures in kJmol1, and in each case state whether the reaction is spontaneous or not under standard conditions.
(Values for Sθin J K–1 mol–1: Ag2CO3(s) = 167.4,
Ag2O(s) = 121.3, CH4(g) = 186.2, Cl2(g) = 165,
CO2(g) = 213.6, H2(g) = 130.6, HCl(g) = 186.8,
H2O(l) = 69.9, Mg(s) = 37.2, MgCl2(s) = 89.6,
Na(s) = 51.2, Na2O2(s) = 95.0, O2(g) = 205.0)
a. H2(g) + Cl2(g) → 2HCl(g) ΔHθreaction=–184.6 kJ mol–1
b. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔHθreaction=–890.3 kJ mol–1
c. 2Na(s) + O2(g) → Na2O2(s) ΔHθreaction=–510.9 kJ mol–1
d. Mg(s) + Cl2(g) → MgCl2(s) ΔHθreaction=–641.3 kJ mol–1
e. Ag2CO3(s) → Ag2O(s) + CO2(g) ΔHθreaction=+167.5 kJ mol–1
Step by Step Answer:
Cambridge International AS And A Level Chemistry Coursebook
ISBN: 9781316637739
2nd Edition
Authors: Lawrie Ryan, Roger Norris