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Total questions: 15
Worksheet time: 15mins
How would the equilibrium shift in the reaction CH4 (g) + 2 H2S (g) <--> CS2 (g) + 4 H2 (g) if the concentration of CH4 was DECREASED?
Left ; toward reactants
Right ; toward products
no change
How would the equilibrium shift in the reaction CH4 (g) + 2 H2S (g) <--> CS2 (g) + 4 H2 (g) if the concentration of H2S was DECREASED?
Left ; toward reactants
Right ; toward products
no change
How would the equilibrium shift in the ENDOTHERMIC reaction CH4 (g) + 2 H2S (g) <--> CS2 (g) + 4 H2 (g) if the temperature was INCREASED?
Left ; toward reactants
Right ; toward products
no change
Which location would generate the most products for an exothermic reaction?
On a table at room temperature
In an oven at a higher temperature
On ice at a lower temperature
How would the equilibrium shift in the reaction CH4 (g) + 2 H2S (g) <--> CS2 (g) + 4 H2 (g) if the concentration of CS2 was INCREASED?
Left ; toward reactants
Right ; toward products
no change
How could volume be changed to favor products in the reaction CH4 (g) + 2 H2S (g) <--> CS2 (g) + 4 H2 (g)
Decrease V
Increase V
impossible
When does Q = K
At equilibrium
When there are more products
When there are more reactants
When is Q < K
At equilibrium
When there are more products
When there are more reactants
When is Q > K
At equilibrium
When there are more products
When there are more reactants
Which reaction would shift toward products if temperature was increased
H2 + Cl2 <--> 2 HCl + 49.7 kJ
2 NH3 + 37.2 kJ <--> N2 + 3 H2
CO + H2O <--> CO2 + H2 + 27.6 kJ
Which reaction would shift toward reactants if volume was decreased
2 H2O (g) + N2 (g) <--> 2 H2 (g) + 2 NO (g)
SiO2 (s) + 4 HF (g) <--> SiF4 (g) + 2 H2O (g)
CO (g) + H2 (g) <--> C (s) + H2O (g)
How would the equilibrium change for the reaction 4 HCl (g) + O2 (g) <--> 2 H2O (g) + 2 Cl2 (g) if volume was INCREASED
Right ; toward products
Left ; toward reactants
no change
How would the equilibrium change for the reaction 4 HCl (g) + O2 (g) <--> 2 H2O (g) + 2 Cl2 (g) if a catalyst was added
Right ; toward products
Left ; toward reactants
no change
How would the equilibrium change for the reaction 2 HgO (s) <--> Hg (l) + O2 (g) if more HgO was ADDED
Right ; toward products
Left ; toward reactants
no change because HgO is a solid
How would the equilibrium change for the reaction 2 HgO (s) <--> Hg (l) + O2 (g) if the pressure INCREASED
Right ; toward products
Left ; toward reactants
no change
