1. Given the reaction 2SO2(g) + O2(g) <--> 2SO3(g) + energy, a decrease in pressure will cause the equilibrium to shift towards… a) Reactants b) Products c) No shift will occur d) Not enough information is provided in the question 2. Given the reaction 2SO2(g) + O2(g) <--> 2SO3(g) + energy, a decrease in temperature will cause the equilibrium to shift towards…
1. Given the reaction 2SO2(g) + O2(g) <--> 2SO3(g) + energy, a decrease in pressure will cause the equilibrium to shift towards…
a) Reactants
b) Products
c) No shift will occur
d) Not enough information is provided in the question
2. Given the reaction 2SO2(g) + O2(g) <--> 2SO3(g) + energy, a decrease in temperature will cause the equilibrium to shift towards…
a) Reactants
b) Products
c) No shift will occur
d) Not enough information is provided in the question
3. Given the reaction 2SO2(g) + O2(g) <--> 2SO3(g) + energy, increasing the concentration of SO3 will cause the equilibrium to shift towards…
a) Reactants
b) Products
c) No shift will occur
d) Not enough information is provided in the question
4. Given the reaction 2SO2(g) + O2(g) <--> 2SO3(g) + energy, adding a potassium iodate inhibitor will cause the equilibrium to shift towards…
a) Reactants
b) Products
c) No shift will occur
d) Not enough information is provided in the question
5. Given the reaction 2SO2(g) + O2(g) <--> 2SO3(g) + energy, adding water to the reaction will cause the equilibrium to shift towards…
a) Reactants
b) Products
c) No shift will occur
d) Not enough information is provided in the question
6. What is the equilibrium constant equation for the reaction 2A(s) + B(g) <--> 2C(g)?
a) K= [C]/[A][B]
b) K= [C]2/[A]2[B]
c) K= [A][B]/[C]
d) None of the above
7. If the equilibrium constant for the forward reaction is K=1000 then the equilibrium constant for the reverse reaction is
a) K=1000
b) K=1
c) K=0.001
d) K=-1000
8. If H=-180kJ/mol and S=45J/k, then the reaction will be…
a) Spontaneous at all temperatures
b) Non-spontaneous at all temperatures
c) Spontaneous at low temperatures
d) Spontaneous at high temperatures
9. If H=-180kJ/mol and S=45J/K, the temperature where an equilibrium reaction will proceed is at…
a) 273K
b) 0K
c) -0.25K
d) -4K
10. In titrations, the point at which the number of moles of acid equals the number of moles of base is known as which of the following?
a) Titrant Zone
b) Indicator
c) Equivalence Point
d) Strong Acid – Strong Base Point
Step by step
Solved in 4 steps with 3 images
