Equilibrium Module 3

Course Name:  Chemistry
Course No.132 NT
Teacher:  Bill Cook
Teacher's Email:  bcook@icc.edu

No. of Questions= 3


1.  Consider the reaction

S2Cl2(l)  +  CCl4(l)  dblaro.jpg (896 bytes) CS2(g)  +  3 Cl2(g)            DH = +84.3 kJ

If the above reactants and products are contained in a closed vessel and the system is at equilibrium, the number of moles of CS2 can be decreased by:

a) adding some S2Cl2 to the system.
b) removing some Cl2 from the system.
c) decreasing the size of the reaction vessel.
d) increasing the temperature of the reaction system.
e) adding some CCl4 to the system.
2.  The equilibrium constant, Kc , for the synthesis of methanol, CH3OH,

CO(g) + 2 H2(g) dblaro.jpg (896 bytes)CH3OH(g)

is 4.3 at 250oC and 1.8 at 275oC. Is this reaction endothermic or exothermic?

a) endothermic
b) exothermic
3.  If the system

NH4Cl(s) dblaro.jpg (896 bytes) NH3(g)  +  HCl(g)

is at equilibrium at constant temperature, and the number of moles of NH4Cl in the vessel is doubled, then:

a) the amount of NH3 and HCl is doubled.
b) the equilibrium amount of NH3 and HCl is incresed.
c) the partial pressure of NH3 and HCl increases until equilibrium is reached.
d) the partial pressure of NH3 and HCl in the vessel remains unchanged.
e) the number of moles of NH4 decreases.



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