Chemical Equilibrium Set 3

Results

#1. Extent to H2 + I2 ® 2HI can be increased by

increasing pressure

increasing product

increasing temp

adding a catalyst

#2. Strength of an acid can be determined by

PKa

PKp

POH

PKw

#3. In an exothermic reversible reaction increase in temp shifts the equilibrium to

reactant side

product side

remains unchanged

none

#4. Units of Kw are

mole dm–3

mole2 dm–3

mole2 dm–6

mole2 dm–3

#5. A basic Buffer solution can be prepared by mixing

weak acid and its salt with strong base

strong acid and its salt with weak base

weak base and its salt with strong acid

strong base and its salt with weak acid

#6. Buffer action can be explained by

common ion effect

law of mass action

Le–Chatlier’s principle

all above

#7. Ionization of weak acid is expressed in term of following constant

#8. Solubility of Ca(OH)2 is exothermic. If solubility will increase

at high temp

at low temp

temp independent

none

#9. For which system does the equilibrium constant, Kc has units of concentration

N2 + 3H2 2NH3

H2 + I2 2 HI

2NO2 N2O4

2HF H2 + F2

#10. Which statement about the following equilibrium is correct 2SO2(g) + O2(g) 2SO3(g) D H = – 188.3 kJ mol–1

the value of Kp falls with a rise in temp

the value of Kp falls with increasing pressure

adding V2O5 catalyst increase the equilibrium yield of sulphur trioxide

the value of Kp is equal to Kc

Finish