Use Lee Chateliers principle to explain went the equilibrium vapor pressure of a

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Use Lee Chateliers principle to explain went the equilibrium vapor pressure of a liquid increases with increasing temperature

Use Lee Chateliers principle to explain went the equilibrium vapor pressure of a liquid increases with increasing temperature


Heating the solution shifts the equilibrium to the right, forming Cooling the solution shifts the equilibrium to the left, toward more blue CoCl4 pink Col0),2 oracg GIVE IT SOME THOUGHT Use Le Châtelier's principle to explain why the equilibrium vapor pressure uid increases with increasing temperature. of aliç reaction, such as Equation 15.23, heat is absorbed as reac ducts. Thus, increasing the temperature causes th tants are converted to pro equilibrium to shift to the right, in the direction of Equation 15.23, increas CoCl4, as observed in Figure 15.14(b). products, and K increases. ing the temperature leads to the formation of mor In an exothermic reaction the opposite occurs, E re converted to reactants; therefore the equilibriu Heat is absorbed as produ ollows: mmarize these res

Explanation / Answer

According to Le Chateliers principle "If any chemical reaction is at equilibrium, any change imposed at equilibrium such as temperature, pressure, concentration etc, the equilibrium will shift to counteract the change".

As the kinetic energy of a molecule is directly proportional to temperature, increase in temperature would also increase the kinetic energy of the molecule. As the kinetic energy increase, the equilibrium will counteract the change by shifting the liquid-vapor equilibrium towards vapor side. As a result, the number of molecules transitioning into a vapor also increases, thereby increasing the vapor pressure.

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