How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each? (a) 2NH3(g) ⇌ N2(g)+3H2(g) ΔH = 92kJ (b) N2(g) + O2(g) ⇌ 2NO(g) ΔH =181kJ (c) 2O3(g) ⇌ 3O2(g) ΔH = − 285kJ (d) CaO(s) + CO2(g) ⇌ CaCO3(s) ΔH = − 176kJ
How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each? (a) 2NH3(g) ⇌ N2(g)+3H2(g) ΔH = 92kJ
(b) N2(g) + O2(g) ⇌ 2NO(g) ΔH =181kJ
(c) 2O3(g) ⇌ 3O2(g) ΔH = − 285kJ
(d) CaO(s) + CO2(g) ⇌ CaCO3(s) ΔH = − 176kJ
le chatelier principle:
It states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to re-establish an equilibrium. If a chemical reaction is at equilibrium and experiences a change in pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to offset the change.
In an exothermic reaction, rise in temperature favours absorption of heat and hence favours the creation of reactants that leads to shifting of equilibrium toward left and vice-versa in case of endothermic reaction.
Increase of pressure on the system leads to decrease in the volume of vessels, then the equilibrium shifts in a direction, where the number of gaseous components are in smaller amount.
(a) 2NH3(g) ⇌ N2(g)+3H2(g) ΔH = 92kJ
Increase in the temperature shifts the equilibrium to right side.
Decrease in the volume of vessel shifts the equilibrium to left side.
(b) N2(g) + O2(g) ⇌ 2NO(g) ΔH =181kJ
Increase in the temperatur...
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