CH 132 Ch 19

The first law of thermodynamics

A reaction that is spontaneous as written _________.

Of the following, only ____ is not a state function. S H q E T

When a system is at equilibrium __________.

A reversible process is one that _______

Which of the following statements is true?

The thermodynamic quantity that expresses the degree of disorder in a system is______.

For an isothermal process, (delta) =

Which of the following is always positive when a spontaneous process occurs?

The entropy of the universe is ________

The second law of thermodynamic states that

Which of the following statements is false?

Consider a pure crystalline solid that is heated from absolute zero to a temperature above the boiling point of the liquid. Which of the following processes produces the greatest increase in the entropy of the substance?

Which one of the following correctly indicates the relationship between the entropy of a system and the number of different arrangements, W, in the system?

Which reaction produces an increase in the entropy of the system? Ag+ (aq) + Cl- (aq)→AgCl(s) CO2 (s)→ CO2 (g) H2 (g) + Cl2 (g)→2HCl(g) N2 (g) + 3H2 (g)→2NH3 (g) H2O(l)→H2O (s)

Which one of the following processes produces a decrease of the entropy of the system? dissolving sodium chloride in water sublimation of naphthalene dissolving oxygen in water boiling of alcohol explosion of nitroglycerine

Which one of the following processes produces a decrease in the entropy of the system? boiling water to form steam dissolution of solid KCl in water mixing of two gases into one container freezing water to form ice melting ice to form water

∆S is positive for the reaction __________. Pb(NO3)2 (aq) + 2KI(aq) → PbI2 (s) + 2KNO3 (aq) 2H2O(g)→2H2(g) + O2 (g) H2O (g)→H2O(s) NO(g) + O2 (g)→NO2 (g) Ag+ (aq) + Cl- (aq) → AgCl (s)

The entropy change accompanying any process is given by the equation: ∆S = k lnWfinal ∆S = k Wfinal - k Winitial ∆S = k ln(Wfinal / Winitial) ∆S = k final - k initial ∆S = Wfinal - Winitial

Of the following, the entropy of __________ is the largest. a. HCl(l) b. HCl(s) c. HCl(g) d. HBr(g) e. HI (g)

Of the following, the entropy of gaseous __________ is the largest at 25°C and 1 atm. a. H2 b. C2H6 c. C2H2 d. CH4 e. C2H4

∆S is negative for the reaction __________. 2H2O (g) → 2H2 (g) + O2 (g) Mg(NO3)2 (aq) + 2NaOH(aq) → Mg(OH)2 (s) + 2NaNO3 (aq) H2O (l) → H2O (g) C6H12O6 (s) → 6C(s)+6H2 (g)+3O2 (g) NaCl(aq)→Na+ (aq) + Cl- (aq)

∆S is negative for the reaction __________. 2SO2 (g) + O2 (g) → 2SO3 (g) NH4Cl (s) →NH3(g)+HCl(g) PbCl2(s)→Pb2+(aq) + 2Cl- (aq) 2C(s) + O2 (g)→2CO2 (g) H2O (l) → H2O (g)

Which of the following statements is false? a. The change in entropy in a system depends on the initial and final states of the system and the path taken from one state to the other. b. Any irreversible process results in an overall increase in entropy. c. The total entropy of the universe increases in any spontaneous process. d. Entropy increases with the number of microstates of the system.

∆S is positive for the reaction __________. 2H2 (g) + O2 (g)→2H2O(g) 2NO2 (g)→ N2O4 (g) CO2 (g)→CO2 (s) BaF2 (s)→ Ba2+ (aq) + 2F- (aq) 2Hg(l) + O2 (g)→ 2HgO (s)

∆S is positive for the reaction __________. CaO(s) + CO2 (g)→CaCO3 (s) N2 (g) + 3H2 (g)→2NH3 (g) 2SO3 (g)→2SO2 (g) + O2 (g) Ag+ (aq) + Cl- (aq) → AgCl (s) H2O (l) → H2O (s)

For an isothermal process, the entropy change of the surroundings is given by the equation: ∆S=qsys T ∆S=-qsys T ∆S=qlnT ∆S=-qlnT ∆S=-qsys /T

Which reaction produces a decrease in the entropy of the system? CaCO3 (s)→CaO(s) + CO2 (g) 2C(s) + O2 (g)→2CO(g) CO2 (s)→CO2 (g) 2H2 (g) + O2 (g)→2H2O(l) e. H2O(l)→ H2O (g)

With thermodynamics, one cannot determine...

The standard Gibbs free energy of formation of __________ is zero. (a) H2O (l) (b) O (g) (c) H2 (g) a. (a) only b. (b) only c. (c) only d. (b) and (c) e. (a), (b), and (c)

Processes that are spontaneous in one direction are ______ in the reverse direction

Spontaneous processes are _____

As a result of all spontaneous processes, the entropy of the universe _______.

Entropy _______ with the number of microstates in the system.

When a solid is dissolved in a solvent, entropy _______.

Standard entropies tend to __________ with increasing molar mass.

When (delta) G is negative, a process is ________.

For a process to be reversible, it must always be in a state...?

in reality, all processes are _______.

The Third law of thermodynamics