# Equilibrium/LeChatelier's Principle: Question Preview (ID: 8709)

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What is a property of a reaction that has reached equilibrium?
a) The amount of products is greater than the amount of reactants
b) The amount of products is equal to the amount of reactants
c) The rate of the forward reaction if greater than the rate of the reverse reaction
d) The rate of the forward reaction is equal to the rate of the reverse reaction

Given the reaction at equilibrium: 2CO(g) + O2(g) <-> 2CO2(g) When the reaction is subjected to stress, a change will occur in the concentration of
a) reactants, only
b) products, only
c) both reactants and products
d) neither reactants nor products

In which reaction will the point of equilibrium shift to the left when the pressure on the system is increased?
a) C(s) + O2(g) <-> CO2(g)
b) CaCO3(s) <-> CaO(s) + CO2(g)
c) 2Mg(s) + O2(g) <-> 2MgO(s)
d) 2H2(g) + O2(g) <-> 2H2O(g)

Given the reaction at equilibrium: 2 SO2(g) + O2(g) <-> 2 SO3(g) + heat. Which change will shift the equilibrium to the right?
c) decreasing the pressure
d) increasing the temperature

Given the reaction A2(g) + B2(g) <--> 2AB(g) + heat. An increase in the concentration of A2(g) will
a) decrease the production of AB(g)
b) decrease the frequency of collisions between A2(g) and B2(g)
c) increase the production of B2(g)
d) increase the frequency of collisions between A2(g) and B2(g)

Given the reaction at equilibrium: N2(g) + 3 H2(g) <--> 2 NH3 (g). If the pressure is increased at constant temperature, there will be an increase in the number of moles of
a) NH3 (g), only
b) N2(g), only
c) H2(g), only
d) both N2(g) and H2(g)

Given the equilibrium reaction in a closed system: H2(g) + I2(g) + heat <--> 2 HI(g). What will be the result of an increase in temperature?
a) The equilibrium will shift to the left and [H2] will increase
b) The equilibrium will shift to the left and [H2] will decrease
c) The equilibrium will shift to the right and [HI] will increase
d) The equilibrium will shift to the right and [HI] will decrease

AgCl(s) + heat <--> Ag+(aq) + Cl-(aq). Which change will cause an increase in the amount of AgCl(s)?
a) a decrease in pressure
b) an increase in temperature
c) a decrease in the concentration of Ag+(aq)
d) an increase in the concentration of Cl-(aq)

Given the reaction at equilibrium: 1/2 N2(g) +1/2 O2(g) + 21.6 kJ <--> NO(g). The equilibrium will shift to the right if the
a) temperature increases
b) temperature decreases
c) pressure increases
d) pressure decreases

A reaction will be spontaneous if it results in products that have
a) lower potential energy and less randomness
b) lower potential energy and more randomness
c) greater potential energy and less randomness
d) greater potential energy and more randomness

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