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Chemistry
- Indicate whether the following processes are spontaneous or nonspontaneous. (a) Liquid water freezing at a temperature below its freezing point (b) Liquid water freezing at a temperature above its freezing point (c) The combustion of gasoline (d) A ball thrown into the air (e) A raindrop falling to the ground (f) Iron rusting in a moist atmospherearrow_forwardGiven the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJarrow_forwardSodium reacts violently with water according to the equation Na(s) + H2O() NaOH(aq) + H2(g) Without doing calculations, predict the signs of rH and rS for the reaction. Verify your prediction with a calculation.arrow_forward
- What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the synthesis of ammonia? 3H2(g) + N2(g) 2NH3(g)arrow_forwardDefine the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forwardCalculate Ssurr for the following reactions at 25C and 1 atm. a. C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) H = 2221 kJ b. 2NO2(g) 2NO(g) + O2(g) H = 112 kJarrow_forward
- Enthalpy changes often help predict whether or not a process will be spontaneous. What type of reaction is more likely to be spontaneous: an exothermic or an endothermic one? Provide two examples that support your assertion and one counterexample.arrow_forwardYeast can produce ethanol by the fermentation of glucose (C6H12O6), which is the basis for the production of most alcoholic beverages. C6H12O6(aq) 2 C2H5OH() + 2 CO2(g) Calculate rH, rS, and rG for the reaction at 25 C. Is the reaction product- or reactant-favored at equilibrium? In addition to the thermodynamic values in Appendix L, you will need the following data for C6H12O6(aq): fH = 1260.0 kl/mol; S = 289 J/K mol; and fG = 918.8 kl/mol.arrow_forwardIndicate the sign (positive or negative) of ΔGo at low and high temperatures for each of the following processes: a) NH3(g) + HCl(g) → NH4Cl(s) b) CaCO3(s) → CaO(s) + CO2(g) c) CH3OH(l) → CH3OH(g) ΔHo < 0 Determine what it would be at Low and high b)CaCO3(s)-->CaO(s)+ CO2(g) Ho > 0 Determine what it would be at low and high c)CH3OH(I)-->CH3OH(g) ΔHo > 0 Determine what it would be at low and high d) 2Cl2(g) + 7O2(g) → 2Cl2O7(l) ΔHo > 0 Determine what it would be at low and higharrow_forward
- Which of the following chemical reactions has a negative ΔS? (The reactions are unbalanced as written - you must balance them!) Group of answer choices PCl5(s) + H2O(l) → POCl3(l) + HCl(aq) TiCl4(s) + H2O(g) → TiO2(s) + HCl(g) Ag(s) + H2S(g) + O2(g) → Ag2S(s) + H2O(g) Fe(s) + H2O(l) → Fe3O4(s) + H2(g)arrow_forwardWhich of the following chemical reactions has a negative ΔS? (The reactions are unbalanced as written - you must balance them!) Group of answer choices Fe(s) + H2O(l) → Fe3O4(s) + H2(g) PCl5(s) + H2O(l) → POCl3(l) + HCl(aq) TiCl4(s) + H2O(g) → TiO2(s) + HCl(g) Ag(s) + H2S(g) + O2(g) → Ag2S(s) + H2O(g)arrow_forwardPredict the signs (–, +, or 0) of ΔH and ΔS, in that order, for the process: H 2O( l) → H 2O( s). –, – +, + 0, – None of the above 0, +arrow_forward
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