Which of the following are true statements about equilibrium systems? False For the following reaction at equilibrium: H2(g) + F2(g) = 2HF(g) removing H2 will decrease the amount of F2 present once equilibrium is reestablished. True For the following reaction at equilibrium: CaCO3(s) = CaO(s) + CO2(g) adding more CaCO3 will shift the equilibrium to the right. True Increasing the temperature of an endothermic reaction shifts the equilibrium position to the right. False For the following reaction at equilibrium: CaCO3(s)= Ca0(s) + CO2(g) increasing the total pressure by adding Ar(g) will shift the equilibrium to the right. True For the following reaction at equilibrium: 2 H2(g) + 02(g) = 2 H20(g) the equilibrium will shift to the left if the volume is doubled. Submit Answer You have entered that answer before Incorrect. Tries 9/99 Previous Tries

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.

For the following reaction, write the equilibrium constant expression and indicate the units Sulfur dioxide reacts with oxygen to produce sulfur trioxide (all are gas phase).

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all?

For an endothermic reaction at equilibrium, increasing the temperature does what?

Why can an equilibrium be represented mathematically? Please explain!

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all?

Expline Fundamental equilibrium concepts and it consisted of the  explain Le Chatelier’s principle to predict the shift of equilibrium

The correct equilibrium expression for the reaction of sulfur dioxide gas with oxygen gas to produce sulfur trioxide gas is

The equilibrium constant changes when...   a a catalyst is added. b the temperature changes. c the surface area changes. d the concentration of reactants changes e more than one above is correct