The following questions (13 and 14) refer to the equilibrium shown here: 4NH3(g)
ID: 579746 • Letter: T
Question
The following questions (13 and 14) refer to the equilibrium shown here: 4NH3(g) + 502(g) 4NO(g) + 6H20(g) 12. What would happen to the system if oxygen were added? Explain. a) More ammonia would be produced. b) More oxygen would be produced. c) The equilibrium would shift to the right. d) The equilibrium would shift to the left. e) Nothing would happen 13. What would happen to the system if the pressure were decreased? Explain. a) b) c) d) e) Nothing would happen More oxygen would be produced The water v The ammonia concentration would increase. The NO concentration would increase. apor would become liquid water 14. For a certain reaction at 25.0°C, the value ofK is 1.2 × 10 At 50.0°C the value ofK is 3.4 × 10-1. This means that the reaction is a) exothermic b) endothermic c) never favorable d) more information needed e) none of these (a-d)Explanation / Answer
12.
(c) The equilbrium would shift to the right.
According to Le-Chatlier's principle, increase of concentration of reactants would shift the equilibrium towards righ side to maintain constant equilibrium constant.
13.
(e) NO concentration would increase.
According to Le-chatlier's principle decrease in pressure would shift the equilibrium towards more number of gaseous substances.
14.
(b) Endothermic.
Increase in temperature increases the equilibrium constant. It means that the forward reaction is endothermic. Because according Lechatlier's principle increase in temperature faovurs endothermic reaction.
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