Chem_Sheet_2_1

Chem_Sheet_2_1 - Equilibrium: a forward reaction and a...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Equilibrium : a forward reaction and a reverse reaction proceed at equal rates, and the concentrations of reactants and products remains constant K c = [G] g [H] h … / [A] a [B] b When the equation for a chemical reaction for which the equilibrium constant is K c is reversed : K’ c = 1/K c When the coefficients of an equation are multiplied by a common factor n to produce a new equation: K’ c = (Kc) n When we add the equations for individual reactions, the equilibrium constants are multiplied K p = (P G ) g (P H ) h … / (P A ) a (P B ) b where P is a Partial Pressure K p = K c (RT) Δngas Δngas = (g + h + …) – (a + b + …) R= .08206 L atm mol -1 K -1 A very large K c or K p signifies that a reaction essentially goes to completion (not reversible) A very small K c or K p signifies that the forward reaction only occurs to a slight extent Q = [G] g in [H] h in … / [A] a in [B] b in If Q < K c : a net change occurs in the forward direction If Q > K c : a net change occurs in the reverse direction Le Chatelier’s Principle : When any change in concentration, temperature, pressure, or volume is imposed on a system at equilibrium, the system responds by attaining a new equilibrium condition that minimizes the impact of the imposed change When the external pressure is increased (volume reduced) equilibrium shifts in direction producing the smaller number of moles
Background image of page 1

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

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 2

Chem_Sheet_2_1 - Equilibrium: a forward reaction and a...

This preview shows document pages 1 - 2. Sign up to view the full document.

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