Lecture 8 (Exam 1 Review)

Lecture 8 (Exam 1 Review) - Equilibrium Pressures At 700 K,...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
Equilibrium Pressures y At 700 K, K p = 0.140 for the reaction: { ClF 3 (g) ClF (g) + F 2 (g) y Calculate the equilibrium partial pressures of all molecules if only ClF 3 is present initially, at a partial pressure of 1.47 atm. What is the total pressure at equilibrium?
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Equilibrium Practice y At a certain temperature, the reaction: { PCl 5 (g) PCl 3 (g) +Cl 2 (g) y Has an equilibrium constant of 5.8 x 10 -2 . Calculate the equilibrium concentrations of all species, if the initial concentrations are initially [PCl 5 ] = 0.200 M, [PCl 3 ] = 0.100 M and [Cl 2 ] = 0.040 M.
Background image of page 2
Equilibrium Problem y The equilibrium constant for the formation of NH 3 is 4.20 at 600 K. When a quantity of gaseous NH 3 was placed in a 1.00 L reaction vessel at 600 K and the reaction was allowed to reach equilibrium, the vessel was found to contain 0.200 mol of N 2 . How many moles of NH 3 were placed in the vessel?
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
y If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change. Henri Louis Le Châtelier
Background image of page 4
Image of page 5
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 12/01/2011 for the course CHEM 105BL taught by Professor Warshel during the Spring '07 term at USC.

Page1 / 12

Lecture 8 (Exam 1 Review) - Equilibrium Pressures At 700 K,...

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online