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1. Hydrogen iodide is placed in a sealed container and allowed to come to equilibrium. The equilibrium reaction is 2HI (g) ↔ H2 (g)+ I2 (g) and the equilibrium concentrations are: [HI]=0,49 M [H2]=1,77 M [I2]=1,77 M Calculate the equilibrium constant. 2. At given temperature, the equilibrium constant for a certain reaction is 1×10-6. Does this equilibrium favor products or reactants? Why? Select the single best answer: Significant concentrations of both products and reactants are present at equilibrium. A very high value for the equilibrium constant favors reactant formation. A very low value for the equilibrium constant favors product formation. A very low value for the equilibrium constant favors reactant formation. A very high value for the equilibrium constant favors product formation. 3. At a given temperature, the equilibrium constant for a certain reaction is 1×1013. Does this equilibrium favor products or reactants? Why? Select a single answer: A small value for the equilibrium constant favors product formation. A large value for the equilibrium constant favors reactant formation. Significant concentrations of both products and reactants are present at equilibrium. A large value for the equilibrium constant favors product formation. A small value for the equilibrium constant favors reactant formation. 4. Select the single best answer: Predict whether a reaction with a negative ΔH and positive ΔS will be spontaneous, nonspontaneous or temperature dependent. nonspontaneous spontaneous temperature dependent 5. Select the single best answer: Determine the sign of ΔG for the following reaction. Is the reaction spontaneous, nonspontaneous or temperature dependent? 42,5 kcal+ CaCO3 (s) ↔ CaO (s) + CO2 (g) nonspontaneous spontaneous temperature dependent 6. Predict whether each of the following processes increases or decreases entropy. Be sure to answer all parts. a) melting of a solid metal b) boiling water 7. Select the single best answer. Is the following process exothermic or endothermic? N2 (g) + 2O2 (g) + 16,2 kcal → 2NO2 (g) endothermic exothermic 8. Select the single best answer. Is the following process exothermic or endothermic? S (s) + 2O2 (g) → SO2 (g), ΔH=-71kcal endothermic exothermic

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Predict whether each of the following processes increases or decreases entropy. Be sure to answer all parts.
a) melting of a solid metal, increases S
b) boiling water, increases S...

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