Interpretation: The effect on equilibrium position of a gas-phase reaction needs to be explained when there is a change in volume of the reaction vessel and whether there are reactions or not that will not shift their equilibria by change in volume needs to be determined. Also, the reason needs to be explained for no shift in equilibrium position for a gas-phase reaction in rigid container to which inert gases are added.
Concept introduction: According to LeChatlier's principle, when a dynamic equilibrium is subjected to a change in either concentration or temperature or pressure, then the position of equilibrium will shift in such a direction that it nullifies the change.
For example:
If concentration of A is increased by adding some more amount of A at equilibrium, then left side concentration is increasing, so to nullify this change, equilibrium shifts towards right side. Hence, forward reaction or formation of C is favoured in this case.
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Chemical Principles
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- What is the difference between homogeneous equilibrium and heterogeneous equilibrium?arrow_forwardFor the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?arrow_forwardAt 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forward
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