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The first law of thermodynamics states that __________ is conserved.

The first law of thermodynamics states that __________ is conserved. matter energy entropy temperature. The first law of thermodynamics states that __________ is conserved. matter energy entropy temperature. Entropy is a measure of the __________ of a system. randomness internal energy

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The first law of thermodynamics states that __________ is conserved.

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  1. The first law of thermodynamics states that __________ is conserved. • matter • energy • entropy • temperature

  2. The first law of thermodynamics states that __________ is conserved. • matter • energy • entropy • temperature

  3. Entropy is a measure of the __________ of a system. • randomness • internal energy • temperature • polarity

  4. Entropy is a measure of the __________ of a system. • randomness • internal energy • temperature • polarity

  5. Since entropy is a state function, the change in entropy is equal to its final value __________ its initial value. • plus • minus • multiplied by • divided by

  6. Since entropy is a state function, the change in entropy is equal to its final value __________ its initial value. • plus • minus • multiplied by • divided by

  7. Entropy decreases when: • gases are formed from liquids. • liquids are formed from solids. • solids are formed from gases. • the number of gas molecules increases during a chemical reaction.

  8. Entropy decreases when: • gases are formed from liquids. • liquids are formed from solids. • solids are formed from gases. • the number of gas molecules increases during a chemical reaction.

  9. The third law of thermodynamics states that the entropy of a pure, perfect crystalline substance at absolute zero (0 K) is: • infinite. • increasing. • decreasing. • zero.

  10. The third law of thermodynamics states that the entropy of a pure, perfect crystalline substance at absolute zero (0 K) is: • infinite. • increasing. • decreasing. • zero.

  11. H = enthalpy. S = entropy. T = Kelvin temperature. The Gibbs free energy, G, is: • H + TS • H – TS • H x TS • H / TS

  12. H = enthalpy. S = entropy. T = Kelvin temperature. The Gibbs free energy, G, is: • H + TS • H – TS • H x TS • H / TS

  13. The value of ∆G, the Gibbs free energy change, for a system at equilibrium is: • positive. • negative. • rapidly fluctuating from positive to negative. • zero.

  14. The value of ∆G, the Gibbs free energy change, for a system at equilibrium is: • positive. • negative. • rapidly fluctuating from positive to negative. • zero.

  15. A reaction will be spontaneous at lower temperatures when the sign of DH and DS is

  16. A reaction will be spontaneous at lower temperatures when the sign of DH and DS is

  17. CaCO3(s) CaO(s) + CO2(g) Upon heating, limestone (CaCO3) decomposes to CaO and CO2. Speculate on the sign of DH and DS for this process.

  18. CaCO3(s) CaO(s) + CO2(g) Upon heating, limestone (CaCO3) decomposes to CaO and CO2. Speculate on the sign of DH and DS for this process.

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