{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Chemistry 122: Changing the reaction conditions: Le Châtelier’s Principle

Chemistry 122: Changing the reaction conditions: Le Châtelier’s Principle

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

View Full Document Right Arrow Icon
Chemistry 121 2/28/2014 Changing the reaction conditions: Le Châtelier’s Principle Obtaining the maximum amount of product from a reaction depends on the proper selection of reaction conditions. By changing these conditions, you can either increase or decrease the yield of product. There are 3 ways to alter the equilibrium composition of a gaseous reaction mixture : 1. Changing the concentrations by removing products or adding reactants. 2. Changing the partial pressure of gaseous reactants and products by changing the volume. 3. Changing temperature. The transformation of nitrogen and hydrogen into ammonia (NH 3 ) is of tremendous significance in agriculture, where ammonia-based fertilizers are of utmost importance. 15.7 Le Châtelier’s Principle “If a system at equilibrium is disturbed by a change in temperature, pressure, or the concentration of one of the components, the system will shift its equilibrium position so as to counteract the effect of the disturbance.” Change in Reactant or Product Concentration - A system at dynamic equilibrium is in the state of balance. When concentrations of
Background image of page 1

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

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

{[ snackBarMessage ]}