(a)
Interpretation: The substance with higher entropy from
Concept Introduction: The entropy of any substance is defined by its degree of randomness. It increases with the molecular weight of a substance and its complexity. If concentration and pressure increase, the entropy of the substance decreases. Also, it depends on the state of the substance. For example, solid substances have less entropy as compared to liquid and gaseous substances that have maximum entropy. For substances in the same state, the substance with higher molecular weight has greater entropy.
(b)
Interpretation: The substance with higher entropy from
Concept Introduction: The entropy of any substance is defined by its degree of randomness. It increases with the molecular weight of a substance and its complexity. If concentration and pressure increase, the entropy of the substance decreases. Also, it depends on the state of the substance. For example, solid substances have less entropy as compared to liquid and gaseous substances that have maximum entropy. For substances in the same state, the substance with higher molecular weight has greater entropy.
(c)
Interpretation: The substance with higher entropy from
Concept Introduction: The entropy of any substance is defined by its degree of randomness. It increases with the molecular weight of a substance and its complexity. If concentration and pressure increase, the entropy of the substance decreases. Also, it depends on the state of the substance. For example, solid substances have less entropy as compared to liquid and gaseous substances that have maximum entropy. For substances in the same state, the substance with higher molecular weight has greater entropy.
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Chemistry: The Molecular Nature of Matter and Change
- For each pair of items, tell which has the higher entropy and explain why. (a) Item 1, a sample of solid CO2 at -78°C, or item 2, CO2 vapor at 0°C (b) Item I, solid sugar, or item 2, the same sugar dissolved in a cup of tea (c) Item 1, a 100-mL sample of pure water and a 100-mL sample of pure alcohol, or item 2, the same samples of water and alcohol after they have been poured together and stirredarrow_forwardWhich contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.arrow_forwardExplain why each of the following statements is incorrect. (a) Entropy increases in all spontaneous reactions. (b) Reactions with a negative free energy change (rG 0) are product-favored and occur with rapid transformation of reactants to products. (c) All spontaneous processes are exothermic. (d) Endothermic processes are never spontaneous.arrow_forward
- At room temperature, the entropy of the halogens increases from I2 to Br2 to Cl2. Explain.arrow_forwardWhich substance has the higher entropy? (a) a sample of pure silicon (to be used in a computer chip) or a piece of silicon containing a trace of another element such as boron or phosphorus (b) O2(g) at 0 C or O2(g) at 50 C (c) I2(s) or I2(g), both at room temperature (d) one mole of O2(g) at 1 bar pressure or one mole of O2(g) at 0.01 bar pressure (both at 298 K)arrow_forwardDiethyl ether, (C2H5)2O, was once used as an anesthetic. Calculate the entropy change, rS, for the vaporization of ether if its heat of vaporization is 26.0 kJ/mol at the boiling point of 35.0 C.arrow_forward
- Which substance has the higher entropy? (a) dry ice (solid CO2) at 78 C or CO2(g) at 0 C (b) liquid water at 25 C or liquid water at 50 C (c) pure alumina, Al2O3(s), or ruby (ruby is Al2O3 in which some Al3+ ions in the crystalline lattice are replaced with Cr3+ ions) (d) one mole of N2(g) at 1 bar pressure or one mole of N2(g) at 10 bar pressure (both at 298 K)arrow_forwardIdentify each of the processes listed as spontaneous or nons-pontaneous. For each nonspontaneous process, describe the corresponding spontaneous process in the opposite direction. (a) A group of cheerleaders builds a human pyramid. (b) Table salt dissolves in water. (c) A cup of cold coffee in a room becomes steaming hot. (d) Water molecules in the air are converted to hydrogen and oxygen gases. (e) A person peels an orange, and you smell it from across the room.arrow_forwardAccording to Lambert, leaves lying in the yard and playing cards that are in disarray on a table have not undergone an increase in their thermodynamic entropy. Suggest another reason why leaves and playing cards may not be a good analogy for the entropy of a system containing, for example, only H2O molecules or only O2 molecules.arrow_forward
- Without doing a calculation, predict whether the entropy change will be positive or negative when each of the following reactions occurs in the direction it is written. (a) CH3OH(l)+3/2O2(g)CO2(g)+2H2O(g) (b) Br2(l)+H2(g)2HBr(g) (c) Na(s)+l/2F2(g)NaF(s) (d)CO(g)+2H2(g)CH3OH(l) (e) 2NH3(g)N2(g)+3H2(g)arrow_forwardFor each process, predict whether entropy increases or decreases, and explain how you arrived at your prediction. 2 CO2(g) → 2 CO(g) + O2(g) NaCl(s) → NaCl(aq) MgCO3(s) → MgO(s) + CO2(g)arrow_forwardCompare the compounds in each set below and decide which is expected to have the higher entropy. Assume all are at the same temperature. Check your answers using data in Appendix L. (a) HF(g), HCl(g), or HBr(g) (b) NH4Cl(s) or NH4Cl(aq) (c) C2H4(g) or N2(g) (two substances with the same molar mass) (d) NaCl(s) or NaCl(g)arrow_forward
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