a)
Interpretation:
The effect of increasing the temperature on the system has to be predicted.
Concept introduction:
Law of mass action: The rate of
Le-Chatelier’s principle: If an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium position.
b)
Interpretation:
The effect of decrease pressure on the given reaction system has to be predicted.
Concept introduction:
Law of mass action: The rate of chemical reaction is directly proportional to the product of concentrations of reactant to products.
Le-Chatelier’s principle: If an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium position.
c)
Interpretation:
The effect of adding
Concept introduction:
Law of mass action: The rate of chemical reaction is directly proportional to the product of concentrations of reactant to products.
Le-Chatelier’s principle: If an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium position.
d)
Interpretation:
The effect of adding catalyst on the given reaction system has to be predicted.
Concept introduction:
Law of mass action: The rate of chemical reaction is directly proportional to the product of concentrations of reactant to products.
Le-Chatelier’s principle: If an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium position.
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Chemistry
- Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forwardWrite an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardAt a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?arrow_forward
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