Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: reaction at 298.15K and 10.6 bars: l2 (s) + H2 (g) à༎ 2HI (g) Using the data in the data section, you calculate the reaction Gibbs free energy change for three moles of iodine and three moles of hydrogen at 298.15K and 10.6 bars to be: a) - 12.0 kJ b) - 7.6 kJ c) - 7.4 kJ d) - 5.8 kJ e) 19.4 kJ f) 20.4 kJ g) 27.8 kJ h) 31.2 kJ Show your calculations! Question 6: (5 points) Consider the following chemical reaction at 1 b0 SI d) – 750 SI e) 1300 SI f) 2400 SI g) – 2400 SI h ) – 1300 SI Make sure you derive the equation used to calculate the change in chemical potential! Question 12: (5 points) o Exactly two moles of substance Y in the liquid state are placed in an empty 0.5 L- containe...
View Full Document

This note was uploaded on 01/26/2014 for the course CHEM 3615 taught by Professor Aresker during the Spring '07 term at Virginia Tech.

Ask a homework question - tutors are online