lechautaliersprinciple

lechautaliersprinciple - • adding CaCO3 o no effect, it's...

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Le Châtelier’s Principle  - equilibrium position changed when outside force disturbs the system affected by concentration, temperature, pressure change in reactant/product concentration >> reaction shifts to use up the added substance lower volume, higher pressure >> reaction shifts to produce less moles of gas higher volume, lower pressure >> reaction shifts to produce more moles of gas higher temperature >> reaction shifts to use up extra energy (depends on whether reaction is exothermic/endothermic) catalysts - only changes how fast equilibrium is achieved, not characteristics of equilibrium itself Describe the effect on CaCO3(s) >> CaO(s) + CO2(g) when:   pressure increased o shifts so that less gas is produced o shifts left volume increased o same as decreasing the pressure o shifts right to produce more gas
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Unformatted text preview: • adding CaCO3 o no effect, it's a solid For reaction PCl5(g) >> PCl3(g) + Cl2(g), K = 0.015 and DH = -375. What happens when Cl2 is removed? • disregard K or DH o they have nothing to do w/ the problem • reaction shifts right to produce more Cl2 For endothermic equation N2(g) + O2(g) >> 2NO(g), K = 4.0 x 10-4. What happens when pressure is increased? • again, disregard K • same amount of moles of gas on both sides of equation • reaction doesn't shift to either side For endothermic equation N2(g) + O2(g) >> 2NO(g), K = 4.0 x 10-4. What happens when temperatre is increased? • N2(g) + O2(g) + energy >> 2NO(g) • adding temperature >> adding energy • reaction shifts right to use up energy...
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This document was uploaded on 10/30/2011 for the course CHEM 161 at Rutgers.

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