Le Chatelier's
1. OBJECTIVE
1.1 To use Le Chatelier’s principle for determining the effect of change in concentration.
1.2 To use Le Chatelier’s principle for determining the effect of change in temperature.
2. INTRODUCTION
Henry-Louis Le Chatelier, (born Oct. 8, 1850, Paris, France—died Sept. 17, 1936, Miribel-les-Échelles), French chemist who is best known for Le Chatelier’s principle, which makes it possible to predict the effect a change of conditions (such as temperature, pressure, or concentration of reaction components) will have on a chemical reaction. His principle proved invaluable in the chemical industry for developing the most-efficient chemical processes.
The most remarkable feature of a system at equilibrium is its ability to return to equilibrium after a change in conditions moves it away from the state. this drive to reattain equilibrium is state in Le Chatelier’s principle: when a chemical system at equilibrium is disturbed, it reattain equilibrium by undergoing a net reaction that reduce the effect of the disturbance.
Two phrases in this statement need further explanation. First, what does it means to ‘disturb’ a system? At equilibrium, Q equals K. When a change in conditions forces the system temporarily out of equilibrium (Q, we say that the system has been disturbed or stresses. Three common disturbances are a change in concentration of a component (that appears in Q), a change in pressure (caused by a change in volume), or a change in temperature.
The other phrase, “net reaction,” is often referred to as a shift in the equilibrium position of the system to the right or left. The equilibrium position is just the specific equilibrium concentrations (or pressures). A shift in the equilibrium position to the right means that there is the net reaction to the right (reactant to product) until equilibrium is reaatained; a shift to the left means that there is a net reaction to the left (product to reactant). Thus, when the disturbance occurs, we say
1.1 To use Le Chatelier’s principle for determining the effect of change in concentration.
1.2 To use Le Chatelier’s principle for determining the effect of change in temperature.
2. INTRODUCTION
Henry-Louis Le Chatelier, (born Oct. 8, 1850, Paris, France—died Sept. 17, 1936, Miribel-les-Échelles), French chemist who is best known for Le Chatelier’s principle, which makes it possible to predict the effect a change of conditions (such as temperature, pressure, or concentration of reaction components) will have on a chemical reaction. His principle proved invaluable in the chemical industry for developing the most-efficient chemical processes.
The most remarkable feature of a system at equilibrium is its ability to return to equilibrium after a change in conditions moves it away from the state. this drive to reattain equilibrium is state in Le Chatelier’s principle: when a chemical system at equilibrium is disturbed, it reattain equilibrium by undergoing a net reaction that reduce the effect of the disturbance.
Two phrases in this statement need further explanation. First, what does it means to ‘disturb’ a system? At equilibrium, Q equals K. When a change in conditions forces the system temporarily out of equilibrium (Q, we say that the system has been disturbed or stresses. Three common disturbances are a change in concentration of a component (that appears in Q), a change in pressure (caused by a change in volume), or a change in temperature.
The other phrase, “net reaction,” is often referred to as a shift in the equilibrium position of the system to the right or left. The equilibrium position is just the specific equilibrium concentrations (or pressures). A shift in the equilibrium position to the right means that there is the net reaction to the right (reactant to product) until equilibrium is reaatained; a shift to the left means that there is a net reaction to the left (product to reactant). Thus, when the disturbance occurs, we say