Q.1
Which of the following would NOT be a determinant of demand?
  • The price of related goods
  • Income
  • Tastes
  • The prices of the inputs used to produce the good
Q.2
What is the Kc expression for this reaction? 2 NO(g) + O2(g) ⇌ 2 NO2(g)
  • Kc = [NO2]2 / [NO]2 [O2]
  • Kc =  [NO]2 [O2] / [NO2]2
  • Kc = [NO]2 [O2] [NO2]2
  • Kc = [NO2]2 / [NO]2 +  [O2]
Q.3
2SO2(g)+O2(g)⇌2SO3(g)Removing O2(g) will
  • shift equilibrium right
  • shift equilibrium left
  • increase pressure
  • have no change
Q.4
A higher price for batteries would tend to
  • increase the demand for flashlights.
  • decrease the demand for electricity.
  • increase the demand for electricity.
  • increase the demand for batteries.
Q.5
H2(g)+Cl2(g)⇌2HCl(g)Removing Cl2(g) will
  • shift equilibrium right
  • shift equilibrium left
  • increase pressure
  • have no change
Q.6
For the reaction...H2 (g) + Cl2 (g) <=> 2HCl (g) + heatIf the pressure in the system is increased, the equilibrium position will _______.
  • shift to the left
  • shift to the right
  • not shift position at all as 2 mol gas <=> 2 mol gas
Q.7
When Q is greater than KcK_cKc​
  • the [Reactants] will increase and [Products] will decrease
  • the [Reactants] will decrease and [Products] will increase
  • the [Reactants] and [Products] will both increase
  • the [Reactants] and [Products] will both decrease
Q.8
The following reaction : SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g) had reached a state of equilibrium, was found to contain 0.mol L-1 SO3 , and 0.mol L-1 NO, 0.mol L-1NO2 , and 0.mol L-1 SOCalculate the equilibrium constant for this reaction.
  • 4
  • .42
  • .25
  • 1
Q.9
Le Chatelier's Principle states that.... If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
  • moves to increase the change
  • moves to counteract the change
  • does not change
Q.10
Consider the following reaction: 2SO2(g) + O2(g) <=> 2SO3(g): ΔΗ = -kJ mol -1Which of the following will NOT shift the equilibrium position to the right?
  • Adding more O2
  • Adding a catalyst
  • increasing the pressure
  • Lowering the temperature
Q.11
For the reaction...N+ O<=> 2NO: Δ H = +kJ mol-1.If the temperature is increased the equilibrium position will shift _______.
  • to the left
  • to the right
  • to the left and right
  • neither left nor right
Q.12
For the reaction...N2 (g) + 3 H2 (g) <=> 2 NH3 (g)If the pressure in the system is increased, which substance(s) will increase in concentration?
  • N2  (as 2 mol gas  → 4 mol gas)
  • H2 (as 2 mol gas  → 4 mol gas)
  • N2 and H2 (as 2 mol gas  → 4 mol gas)
  • NH3 (as 4 mol gas  → 2 mol gas)
Q.13
For the reaction...SO2 + O<=> SO3If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
  • to the left
  • to the right
  • to the left and right
  • neither left nor right
Q.14
For the reaction...SO2 + O2 <=> SO3If the equilibrium position shifts to the right, the concentration of O2 will ___________.
  • increase
  • decrease
  • remain the same
  • double
Q.15
For the reaction...N+ O<=> 2NOIf O2 is removed, the concentration of N2 will _______.
  • increase
  • decrease
  • remain the same
  • double
Q.16
If a salt solution is at equilibrium, it is
  • unsaturated
  • saturated
  • super-saturated
  • salty
Q.17
What is equal in an equilibrium reaction?
  • concentrations
  • rates
  • moles
  • masses
Q.18
In a system at equilibrium
  • the forward reaction stops
  • the reverse reaction stops
  • both reactions stop
  • both reactions continue at the same rate
Q.19
If the concentration of a chemical is increased by adding more of it to a system at equilibrium, its concentration will _________________ to get the system back to equilibrium.
  • decrease
  • stay the same
  • increase
  • get completely used up
Q.20
The units of concentration used in equilibrium constant expressions is
  • molality
  • molarity
  • % concentration by mass
  • ppm
0 h : 0 m : 1 s