Observe the following process: LiBr_(s) LiBr_(aq), delta H_soln = -49.0 k3/mol W
ID: 529255 • Letter: O
Question
Observe the following process: LiBr_(s) LiBr_(aq), delta H_soln = -49.0 k3/mol We increase the temperature of the solution. In which direction will the reaction shift? The following reaction happens in a 1.5 L flask. N_2(g) + 3 H_2(g) 2 NH_3(g) If the reaction mixture is expanded into a 4L flask, in which direction does the reaction shift? Observe the following reaction: 2 SO_2(s) + O_2(s 2 SO_3(s) SO_2 is added to the reaction mixture. In which direction does the reaction shift? Observe the following reaction: H_2(g) + I_2(g) 2 HI_(g)Explanation / Answer
(70)
According to Lechatlier's principle,
Increase in temperature favours the endothermic reaction i.e the reaction that absorbs energy.
Since in the given example back ward reaction is endothermic, increase in temperature shits the equilibrium towards left side.
(71) According to Lecahtlier's principles, increase in volume shifts the equilibrium otwards more number of gas moles.
IN the given examples, number of gas moles of reactants = 4 and that of products = 2
Hence increase in volume shifts the equilibrium towards left side.
(72) According to Lechatlier's principle, addition of reactants or removal of products shifte the equilibrium towards right side.
Since, SO2 is one of the reactants, addition of SO2 shifts the equilibrium towards right side.
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