Free Energy Reactants Progress of Reaction Products Choose all options that apply to the above graph Gibb's Free Energy is decreasing This graph shows a reaction that would be spontaneous at this temperature Gibb's Free Energy is increasing This graph shows an endergonic reaction

The A,G° for the following reaction is - 100.4 kJ. C2H4(g) + H2(g) –→ C2H6(g) Given A;G° [C2H4(g)] = +68.4 kJ/mol, calculate AG° [C2H6(8]. -168.8 kJ/mol-rxn +32.0 kJ/mol-rxn +1.486 kJ/mol-rxn -32.0 kJ/mol-rxn +168.8 kJ/mol-rxn

7. What is true about the spontaneity of a reaction?     a.When the products have less enthalpy than the reactants, the reaction tends to be spontaneous.   b.When the products have less enthalpy than the reactants, the reaction is always spontaneous.   c.When the products have more enthalpy than the reactants, the reaction tends to be spontaneous.   d.When the products have more enthalpy than the reactants, the reaction is always spontaneous.

What is the entropy of a reaction? What does it mean when the entropy increases? What kinds of reactions contribute to an increase in entropy?

QUESTION 3 A glass of water at room termperature is an example of: O 1st Law of Thermodynamics O Zeroth Law of Thermodynamics O 3rd Law of Thermodynamics O 2nd Law of Thermodynamics

When global temperatures rise, ocean evaporation increases water vapor in the air, water vapor in the air acts as a greenhouse gas trapping heat in the atmosphere and global temperatures increased. This is an example of: 1. Negative feedback loop 2. positive feedback loop 3. not a feedback loop.

Hydrated copper(II) sulfate crystals were heated: What is the ice for?   What color change will occur in the test-tube? pale blue to white.  The reaction is reversible. What does that mean? This means that the products can change back to the original form.  How would you show that it is reversible?  Write the equation for the reversible reaction.

Which of the following circumstances will result in a reaction that is spontaneous only at low temperatures? positive enthalpy change and positive entropy change negative enthalpy change and negative entropy change positive enthalpy change and negative entropy change negative enthalpy change and positive entropy change

Consider the following reaction at equilibrium. NH3 + H₂O NH4+ + OH- Which of the following statements would be correct if the NH3 was removed? the rate of formation of ammonia would stay the same the rate of formation of ammonia would decrease the rate of formation of hydroxide would stay the same removing of the NH3 is not possible as it violates the second law of thermodynamics

0 Question 26 Which illustration shows an energy diagram for an exothermic reaction with three steps? L O free energy kJ/mol D OB OC O A reaction coordinate A reaction coordinate B. reaction coordinate C. reaction coordinate D.