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Chapter 17
Free Energy and Thremodynamics
| Question | Answer |
|---|---|
| There is a 'heat tax' | for every energy transaction |
| The _______________ Law of Thermodynamics sates the energy is conserved in chemical processes. | First |
| Identify the process that is spontaneous. | rusting of iron |
| __________________ is a thermodynamic function that increases w/ the number of energetically equivalent ways to arrange components of a system to achieve a particular state. | Entropy |
| The ________________ Law of Thermodynamics states that for any spontaneous reaction, the entropy of the universe increase. | Second |
| Which of the following processes have a Δs>0? | CH4(g) + H2O(g) --> Co(g) + 3 H(g) |
| Endothermic processes decrease | the entropy of the surroundings, at constant T and P. |
| What is the sign of ΔSuniv for a biological system? | positive |
| Which of the following relationships is correct at constant T and P? | ΔG is proportional to -ΔSuniv |
| Consider a reaction that has a positive ΔH and a positive ΔS. | This reaction will be spontaneous only at high temps and nonspontaneous at low temps |
| Consider a reaction that has a negative ΔH and a positive ΔS. | This reaction will be spontaneous at all temps |
| Consider a reaction that has a positive ΔH and a negative ΔS. | This reaction will be nonspontaneous at all temps |
| Consider a reaction that has a negative ΔH and a negative ΔS | This reaction will be nonspontaneous only at high temps This reaction will be spontaneous at low temp |
| 2 N2O(g) --> 2 N2(g) + O2(g) | a negative ΔH and a positive ΔS |
| 3O2 --> 2O3(g) | a positive ΔH and a negative ΔS |
| H2O --> H2O(g) | a positive ΔH and a positive ΔS |
| H2O --> H2O(s) H2)(I) --> H2O(s) | a negative ΔH and a negative ΔS |
| The _______________ Law of thermodynamics states the entropy of a perfect crystal at absolute zero is is zero. | Third |
| For a given compound, list the decreasing order of entropy for a liquid. solid. and gas. | gas>liquid>solid |
| Entropy is | an extensive property |
| Free atoms have | greater entropy than molecules |
| What can change the direction of a reversible reaction? | change in temp, pressure, volume |
| Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics | reversible reaction |
| If ΔGrxn>0 | the reaction is spontaneous in the forward direction |
| ΔGrxn=0 | at equilibrium |
| ΔGrxn is positive and the reaction | is spontaneous in the reverse direction |
| ΔGrxn is negative and the reaction | is spontaneous in the forward direction |
| ΔGrxn is zero and the reaction | is at equilibrium |
| Which of the following reactions will have the largest equilibrium constant (K) at 298K? | 2 Hg(g) + O2(g) --> 2HgO(s) ΔG=-180.8 kJ |
| In which of the following processes does the molecules become more orderly? Identify the change in state that does not have an increase in entropy. | water freezing |
| Which of the following processes have a ΔS>0? | potassium iodide dissolves in pure water |
| Which of the following processes have a ΔS<0? | water freezes, methyl alcohol condenses, propanol (g, at 555 K) --> propanol (g, at 400 K) CO2 (g) --> CO2 (s) |
| Which of the following processes shows a decrease in entropy of the system? | 2 NO (g) + O2 (g) --> 2 NO2 (g) |
| Which one of the following has the highest standard molar entropy, S, at 25C? | I2 (g) |
| Identify the compound that is NOT an allotrope of carbon. | ethanol |
| Which one of the following would be expected to have the lowest standard molar entropy, S an 25C? | C10H22 (s) |
| Identify the compound w/ the lowest standard free energy of formation | NaCl (s) |
| Identify the compound w/ the highest standard free energy of formation | O3 (g) |
| Identify the compound w/ the standard free energy of formation equal to zero. | H2 (g) |
| Q=K | Equilibrium |
| Q<K | DG<0 |
| Q>K | ΔG>0 |
| Q=1 | Standard state |
| Q>1 | ΔG>ΔG |
| Q<1 | ΔG<ΔG |
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