5a) If the pressure was increased, which way would the equilibrium shift? a) to the right b) to the left c) it would not shift 5b) If the temperature is increased, which way would the equilibrium shift? a) to the right b) to the left c) it would not shift 5c) what would happen to the concentration of Na(g)? a) increase b) decrease c) Remain the same

For the following equilibrium reaction; H2 + 12 2HI If you were to remove some H2, the reaction would shift If you were to remove some HI, the reaction would shift

Consider the following reaction at equilibrium: 2H₂S (g) 2H₂(g) + S₂ (g) What would be the direction of the above reaction if we increase the concentration of H₂? The reaction will proceed (shift) to the left The reaction would not be affected. The reaction will proceed (shift) to the right.

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.