Q.1
For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 2.3x10-[H2]= 0.0056mol, [Cl2]= 0.0048mol.
  • 6.2 x 10-10 M
  • 2.5 x 10-5 M
  • 1.1 M
  • 1.2 M
Q.2
What is the correct formula of relationship between Kc and Kp?
  • Kp=Kc(RT)ΔnKp=Kc\left(RT\right)^{\Delta n}Kp=Kc(RT)Δn
  • Kc=Kp(RT)ΔnKc=Kp\left(RT\right)^{\Delta n}Kc=Kp(RT)Δn
  • Kp=(RT)ΔnKp=\left(RT\right)^{\Delta n}Kp=(RT)Δn
  • Kp×Kc=(RT)ΔnKp\times Kc=\left(RT\right)^{\Delta n}Kp×Kc=(RT)Δn
Q.3
What kind of equilibrium does the reaction below show?H2(g) +I2(g) ↔ 2HI(g)
  • Heterogeneous equilibrium, all the reactants and products are in the same physical state.
  • Homogeneous equilibrium, all the reactants and products are in the same physical state.
  • Heterogeneous equilibrium, the reactants and products are present in more than one physical state
  • Homogeneous equilibrium, the reactants and products are present in more than one physical state
Q.4
+ <----> 2ABThe forward reaction forms the substance __________.
  • A
  • B
  • AB
  • A + B
Q.5
For the reaction...heat + N+ O↔ 2NOIf the heat is added to the chemical system, the equilibrium will shift _______.
  • left
  • right
  • left and right
  • neither left nor right
Q.6
For the reaction...N2 (g) + 3 H2 (g) <−> 2 NH3 (g)If the pressure in the system is increased, which substance will increase in concentration?
  • N2
  • H2
  • N2 and H2
  • NH3
Q.7
For the reaction...N2 (g) + 3 H2 (g) <−> 2 NH3 (g)If the pressure in the system is increased, _______ reaction will be favored.
  • the forward
  • the reverse
  • neither
Q.8
For the reaction...H2 (g) + Cl2 (g) <−> 2HCl (g) + heatIf the pressure in the system is increased, the equilibrium will _______.
  • shift left
  • shift right
  • not shift
Q.9
For the reaction...H2 (g) + Cl2 (g) <−> 2HCl (g) + heatIf the temperature is cooled, the _________ reaction will be favored.
  • forward
  • reverse
  • forward and reverse
Q.10
For the reaction...heat + N+ O<−> 2NOIf O2 is removed, the concentration of N2 will _______.
  • increase
  • decrease
  • remain the same
  • double
Q.11
For the reaction...SO2 + O2 <−> SO3If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
  • left
  • right
  • left and right
  • neither left nor right
Q.12
For the reaction...SO2 + O2 <−> SO3If the equilibrium shifts to the right, the concentration of O2 will ___________.
  • increase
  • decrease
  • remain the same
  • double
Q.13
For the reaction...SO2 + O<−> SO3If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
  • left
  • right
  • left and right
  • neither left nor right
Q.14
+ <----> 2ABThe reverse reaction forms the substance __________.
  • A
  • B
  • AB
  • A + B
Q.15
+ <----> 2ABThe reverse reaction points towards the __________.
  • left
  • right
  • up
  • down
Q.16
+ <----> 2ABThe forward reaction points towards the __________.
  • left
  • right
  • up
  • down
Q.17
What is the equilibrium-constant expression for CO2(g) + H2(g) ↔ CO(g) + H2O(l)
  • Kc= [CO][H2O] / [CO2][H2]
  • Kc= [CO2][H2] / [CO]
  • Kc= [CO2][H2] / [CO][H2O]
  • Kc= [CO] / [CO2][H2]
Q.18
Such reactions which continue in both directions are called:
  • Irreversible reactions
  • Reversible reactions
  • Non-reactive reactions
  • dynamic reactions
Q.19
A complete reaction is in which:
  • All the reactants convert into products
  • All the reactants do not convert into products
  • Half reactants convert into products
  • only 10% reactants convert into products
Q.20
2SO2(g)+O2(g)⇌2SO3(g)Adding SO2(g) will
  • shift equilibrium right
  • shift equilibrium left
  • increase rate of reaction
  • have no change
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