problem_set_06 - 6. At a total pressure of 0.02 atm, what...

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

View Full Document Right Arrow Icon
1 Problem Set 6 Chem 110A F09 (THE FIRST 4 PROBLEMS REFER TO DISCUSSION IN LECTURE #18, corresponding to Eqs. (6.22) through (6.35) in the text.) 1. Derive Eqs. (6.22), (6.23) and (6.24). 2. Derive Eqs. (6.26), (6.27) and (6.28). 3. Find the mistake in Eq. (6.34), as written in the textbook. Then show how the correctly written Eq. (6.34) can be written for a chemical reaction by replacing G by G (where G is the Gibbs free energy change for the reaction, G rxn ) and H by H (where H is the enthalphy change for the reaction, H rxn ). Finally, show how this leads to Eq. (6.35). 4. Derive an equation for the temperature-dependence of the Helmholtz free energy A, in analogy to Eq. (6.34) for the temperature-dependence of the Gibs free energy, i.e., obtain a general expression for ( A T 1 T ) V . 5. In deriving the final form of Eq. (6.35), we neglected the temperature-dependence of the enthalpy of reaction. How good an approximation is this?
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 6. At a total pressure of 0.02 atm, what temperature is needed for the reaction Br 2 (g) = 2Br(g) to equilibrate with half the bromine atoms present as atomic bromine? 7. Consider the decomposition reaction NOCl(g) = NO(g) + (1/2) Cl 2 (g). Suppose we start with 4.00 moles of NOCl(g) and allow it to decompose at a temperature of 375K and under a pressure of 1.5 atm. How much reaction occurs when the system has come to equilibrium at this temperature and pressure? (To simplify the algebra, you may want to assume that the extent of decomposition is small; then, after obtaining a solution for the final partial pressures of each component, check that this assumption was indeed a good approximation.) 8. Play some more with the system in problem 7 above, e.g., change the initial amount of NOCl(g), or the pressure, or the temperature, etc. Think about your results in terms of Le Chateliers principle....
View Full Document

This note was uploaded on 04/17/2011 for the course CHEM 110A taught by Professor Schwartz during the Spring '06 term at UCLA.

Ask a homework question - tutors are online