Question

Laboratory 11, Equilibrium Control of a Reaction Name Chemical Equilibrlum: equilibrium is when the rates of the forward and reverse reactions are equal. Therefore, the concentration of all reactants and products remain constant. This is not to say that the reaction has ceased. It is a dynamic situation at chemical equilibrium with the rate of disappearance of reactants the same as the rate of appearance of reactants through the reverse reaction (the same for the rate of disappearance and appearance of products) Common lon: A salt contains an ion that is common to an equilibrium reaction. The common ion can have an impact on the equilibrium of a chemical reaction Le Chatelier's Principle: When a stress is placed upon a system in equilibrium, the system will respond in a manner that will relieve the stress Examine the following equililbrium reaction and use Le Chatelier's Principle to answer the following questions addition0fvanadiumlínions. The stress is an increased concentration of vanadium(IM). The reaction will shift forward, reducing the concentration of v ons The stress is reduced heat. The reaction will shift in reverse to create more heat. The stress is a reduced concentration of Br ions, the reaction will shift forward creating new Br ions oolins the reastion ) Cooling the reaction NaBr consists of Na and Br ions. Br is a common ion in the reaction. Therefore, the addition of NaBr will increase the concentration of Br ions, shifting the reaction forward. v) Addition of NaBr NaCI consists of Na" and Cl ions. Neither are common ions to the reaction. Therefore, NaCI will not place a stress on the reaction. No shift in equilibrium. v) Addition of NaCI

Answer 1

Given reaction CH_4_(g) + ZO_2_(g) rightharpoonoverleftharpoon CO_2_(g) + 2H_2 O_(g) + delta (1) Action a) add CH_4 to the reaction rightarrow as reactant amount is increased so shift right b) add O_2 to the reaction rightarrow as reactant amount is increased so shift right c) Add CO_2 to the reaction rightarrow as product amount is increased so shift left d) add H_2 O to the reaction rightarrow as product amount is increased so shift left e) remove CH_4 from the reaction rightarrow as reactant amount is decreased so shift left f) remove O_2 from the reaction rightarrow as reactant amount is decreased so shift left g) remove CO_2 from the reaction rightarrow as product amount is decreased so shift right h) remove H_2 O from the reaction rightarrow as product amount is decreased so shift right i) Cool the reaction mixture rightarrow Since it is exothermic so at lower temperature shift rigid. i) Hear the reaction mixture rightarrow since it is