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CHEMISTRY LOOSELEAF TEXT W/CONNECT >IP
- Calculate the entropy change for each of these processes. thereby verifying the predictions made in Conceptual Exercise 16.4. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) NaCl(s) NaCl(aq) (c) MgCO3(s) MgO(s) + CO2(g)arrow_forwardPredict the sign of S for each of the following and explain. a. the evaporation of alcohol b. the freezing of water c. compressing an ideal gas at constant temperature d. dissolving NaCl in waterarrow_forwardImpure nickel, refined by smelting sulfide ores in a blast furnace, can be converted into metal from 99.90% to 99.99% purity by the Mond process. The primary reaction involved in the Mond process is Ni(s)+4CO(g)Ni(CO)4(g) a. Without referring to Appendix 4, predict the sign of S for the above reaction. Explain. b. The spontaneity of the above reaction is temperature-dependent. Predict the sign of Ssurr, for this reaction. Explain c. For Ni(CO)4(g), Hfo=607KJ/mol and S = 417 J/K mol at 298 K. Using these values and data in Appendix 4, calculate H and S for the above reaction. d. Calculate the temperature at which G = 0 (K = 1) for the above reaction, assuming that H and S do not depend on temperature. e. The first step of the Mood process involves equilibrating impure nickel with CO(g) and Ni(CO)4(g) at about 50C. The purpose of this step is to convert as much nickel as possible into the gas phase. Calculate the equilibrium constant for the above reaction at 50.C. f. In the second step of the Mood process, the gaseous Ni(CO)4 is isolated and heated to 227C. The purpose of this step is to deposit as much nickel as possible as pure solid (the reverse of the preceding reaction). Calculate the equilibrium constant for the preceding reaction at 227C. g. Why is temperature increased for the second step of the Mood process? h. The Mond process relies on the volatility of Ni(CO)4 for its success. Only pressures and temperatures at which Ni(CO)4 is a gas are useful. A recently developed variation of the Mood process carries out the first step at higher pressures and a temperature of l52C. Estimate the maximum pressure of Ni(CO)4(g) that can be attained before the gas will liquefy at 152C. The boiling point for Ni(CO)4 is 42C and the enthalpy of vaporization is 29.0 kJ/mol. [Hint: The phase change reaction and the corresponding equilibrium expression are Ni(CO)4(l)Ni(CO)4(g)K=PNi(CO)4 Ni(CO)4(g) will liquefy when the pressure of Ni(CO)4 is greater than the K value.]arrow_forward
- Consider two perfectly insulated vessels. Vessel 1 initially contains an ice cube at 0C and water at 0C. Vessel 2 initially contains an ice cube at 0C and a saltwater solution at 0C. Consider the process H2O(s) H2O(l). a. Determine the sign of S, Ssurr, and Suniv for the process in vessel 1. b. Determine the sign of S, Ssurr, and Suniv for the process in vessel 2. (Hint: Think about the effect that a salt has on the freezing point of a solvent.)arrow_forwardIndicate 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_forwardWhich of the following processes are spontaneous? (a) ice cream melting at 75F (b) sorting a list of names alphabetically (c) gathering leaves in a pilearrow_forward
- Use S values to calculate the standard entropy change, rS0, for each of the following processes and comment on the sign of the change. (a) KOH(s) KOH(aq) (b) Na(g) Na(s) (c) Br2() Br2(g) (d) HCl(g) HCl(aq)arrow_forwardEstimate the sign of the entropy change for the reaction: CaCO3 (s) → CaO (s) + CO2 (g) Select one: a. is zero b. negative c. not possible to determine the sign d. none of these e. positivearrow_forwardANSWER PARTS A, B, C, & D A. Which one of the following processes produces a decrease in the entropy of the system? A) boiling water to form steam B) dissolution of solid KCl in water C) mixing of two gases D) freezing water to form ice E) melting ice to form water B. ΔS is positive for the reaction __________. A) 2H2 (g) + O2 (g) → 2H2O (g) B) 2NO2 (g) → N2O4 (g) C) CO2 (g) → CO2 (s) D) BaF2 (s) → Ba2+ (aq) + 2F- (aq) E) 2Hg (l) + O2 (g) → 2HgO (s) C. For the reaction C2H6 (g) → C2H4 (g) + H2 (g) ΔH° is + 137 kJ/mol and ΔS° is +120 J/K ∙ mol. This reaction is __________. A) spontaneous at all temperatures B) spontaneous only at high temperature C) spontaneous only at low temperature D) nonspontaneous at all temperatures D. Which of these processes lead(s) to an increase in entropy? (treat all gases as ideal). Circle all that apply. A) The pressure of 1 mole of oxygen gas is allowed to double isothermally. B) Carbon dioxide is allowed to expand isothermally to 10 times its…arrow_forward
- Find ∆Stotal (entropy change) when 100 grams of water vapor initially at 200 degrees Celsius undergoes a cyclic process for which heat, qtotal = 1450 Joules. Given: 333.6 J/g and 2256.7 J/g as the heats of fusion and vaporization of water, respectively. Group of answer choices ΔS = 3.06 J/K ΔS = 70.51 J/K ΔS = 306.46 J/K ΔS = 476.95 J/K None of thesearrow_forward1. Which set of results applies to a reaction that is spontaneous at 250 K but is not spontaneous at 350 K? A) H<0 and S<0, B) H>0 and S>0, C) none, D) H>0 and S<0arrow_forwardFor which set of conditions is the reaction always nonspontaneous? ΔH = + and ΔS = + ΔH = - and ΔS = - ΔH = - and ΔS = + ΔH = + and ΔS = - ΔH = 0 and ΔS = 0arrow_forward
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