tne oxide, NO(e), and bromine, Bra(g), were allowed to react in a sealed contain

Question

tne oxide, NO(e), and bromine, Bra(g), were allowed to react in a sealed container n equilibrium was r eached, Po 0.526 atm, Par2 1.59 atm, and PNOBr 7.68 atm Calculate the equilibrium A) 0.00746 B) 0.109 C) 9.18 D) 134 The dissociation of a weak acid is endothermic. Which of the following statements is constant for the reaction: 7 true about its percent dissociation? Percent dissociation increases with temperature and increases with concentration. B) Per rcent dissociation increases with temperature but decreases with concentration. C) Percent dissociation decreases with temperature but increases with concentration D) Percent dissociation decreases with temperature and decreases with concentration S. The reaction represented below is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen, PHa, is doubled? A) As equilibrium is re-established, Pes, increases. B) As equilibrium is re-established, Pcn, decreases. C) As equilibrium is re-established, Ph2 decreases. D) As equilibrium is re-established, Phas decreases. 9. Consider the equilibrium reaction represented by the equation: No(g) - 2 NO-() Which of the following expressions corectly describes the relationship between Ke and K, for this reaction? 10. Nitrogen dioxide, NO-(g), can dissociate into nitric oxide, NOK), and oxygen, O-(g), in a reaction represented by the equation: 2 NO2(g) 2 NO g) + 02(g) Under which conditions would you expect to produce the largest amount of oxygen? A) high temperature, high pressure B) high temperature, low pressure C) low temperature, high pressure D) low temperature, low pressure

Explanation / Answer

1. For the reaction 2NO(g)+ Br2(g) ßà 2NOBr(g)

Kp = (PNOBr)2/ (PNO)2*(PBr2), P denotes partial pressure.

=7.68*7.68/(0.526*0.526*1.59)=134 ( D is correct)

2. for endothermic reaction, with an increase in temperature, as per Lechatlier Principle, with an increase in temperature, the reaction should proceed in a direction so as to oppose the increase in temperature, so the reaction proceeds in endothermic direction and this increase the degree of dissociation. since percent dissociation increases, the equilibrium concentration is decreased.

for the reaction, HA +H2O ------>A-+ H3O+

so when HA is increased, to compensate the increased HA, A- and H3O+ wlll have to increase. so % dissociation increases with concentration. ( A is correct)

2. for the reactionm, K = [PCH4][PH2S]2/ [PCS2] [PH2]4

since partial pressure of H2 increased, to keep equilibrium constant, PH2 and PH2S also will increase and when Equilibrium is reestablished, PH2 decreases.( C is correct)

3. the relation between Kp and KC is Kp = KC*(RT) deltan, deltan= change in no of moles during the reactino = 2-1=1

KP= KCRT (B is correct)

4. the reactinois endothermic so hence increase in temperature favors prodducts and hence more O2 is produced.

when pressure is increased, the reaction proceeds in a direction where there is a decrease in no of moles. So forward reaction is preferred. ( A is correct)

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