Question

In: Other

Calculate H298 and S298 for the following reactions: a) 2TiO + ½ O2 = Ti2O3 b)...

Calculate H298 and S298 for the following reactions:
a) 2TiO + ½ O2 = Ti2O3
b) 3Ti2O3 + ½ O2 = 2Ti3O5
c) Ti3O5 + ½ O2 = 3TiO2

Expert Solution

Part a

2TiO + ½ O2 = Ti2O3

Enthalpy change for the reaction = sum of Enthalpy of formation of products - sum of Enthalpy of formation of reactants

H = Hf(Ti2O3) - 0.5*Hf(O2) - 2*Hf(TiO)

= - 1521 - 0 - 2*(-543)

= - 435 kJ/mol

Entropy change for the reaction = sum of Entropy of formation of products - sum of Entropy of formation of reactants

S = Sf(Ti2O3) - 0.5*Sf(O2) - 2*Sf(TiO)

= 77.2 - 0.5*205.1 - 2*(34.7)

= - 94.75 J/mol·K

Part b

3Ti2O3 + ½ O2 = 2Ti3O5

Enthalpy change

H = 2*Hf(Ti3O5) - 0.5*Hf(O2) - 3*Hf(Ti2O3)

= 2*(-2459) - 0 - 3*(-1521)

= - 355 kJ/mol

Entropy change

S = 2*Sf(Ti3O5) - 0.5*Sf(O2) - 3*Sf(Ti2O3)

= 2*(129.4) - 0.5*205.1 - 3*(77.2)

= - 75.35 J/mol·K

Part c

Ti3O5 + ½ O2 = 3TiO2

Enthalpy change

H = 3*Hf(TiO2) - 0.5*Hf(O2) - Hf(Ti3O5)

= 3*(-944) - 0 - (-2459)

= - 373 kJ/mol

Entropy change

S = 3*Sf(TiO2) - 0.5*Sf(O2) - Sf(Ti3O5)

= 3*(50.6) - 0.5*205.1 - (129.4)

= - 80.15 J/mol·K

Amanda K answered 2 years ago

Part A. Calculate the enthalpy of the reaction 2NO(g)+O2(g)?2NO2(g) given the following reactions and enthalpies of...

Part A. Calculate the enthalpy of the reaction 2NO(g)+O2(g)?2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)?NO2(g), ?H?A=33.2 kJ 12N2(g)+12O2(g)?NO(g), ?H?B=90.2 kJ Part B. Calculate the enthalpy of the reaction 4B(s)+3O2(g)?2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)?3O2(g)+B2H6(g), ?H?A=+2035 kJ 2B(s)+3H2(g)?B2H6(g), ?H?B=+36 kJ H2(g)+12O2(g)?H2O(l), ?H?C=?285 kJ H2O(l)?H2O(g), ?H?D=+44 kJ

Part A Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of...

Part A Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔfH∘A=33.2 kJ mol−1 12N2(g)+12O2(g)→NO(g), ΔfH∘B=90.2 kJ mol−1 Express your answer with the appropriate units. Part B Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔrH∘A=+2035 kJ mol−1 2B(s)+3H2(g)→B2H6(g), ΔrH∘B=+36 kJ mol−1 H2(g)+12O2(g)→H2O(l), ΔrH∘C=−285 kJ mol−1 H2O(l)→H2O(g), ΔrH∘D=+44 kJ mol−1 Express your answer with the appropriate units.

Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g),...

Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ

Calculate the enthalpy of the reaction 2NO(g)+O2(g)?2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)?NO2(g), ?H?A=33.2...

Calculate the enthalpy of the reaction 2NO(g)+O2(g)?2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)?NO2(g), ?H?A=33.2 kJ 12N2(g)+12O2(g)?NO(g), ?H?B=90.2 kJ Express your answer with the appropriate units. ?H? = Part B Calculate the enthalpy of the reaction 4B(s)+3O2(g)?2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)?3O2(g)+B2H6(g), ?H?A=+2035 kJ 2B(s)+3H2(g)?B2H6(g), ?H?B=+36 kJ H2(g)+12O2(g)?H2O(l), ?H?C=?285 kJ H2O(l)?H2O(g), ?H?D=+44 kJ Express your answer with the appropriate units. ?H? =

Calculate the equilibrium constant for each of the reactions at 25 ∘C. Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq) Express...

Calculate the equilibrium constant for each of the reactions at 25 ∘C. Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq) Express your answer using two significant figures.

For the following oxidation-reduction reactions, circle the reactant that is oxidized. (a) O2 (g) + 2Cu...

For the following oxidation-reduction reactions, circle the reactant that is oxidized. (a) O2 (g) + 2Cu (s) → 2CuO (s) (b) 2K (s) + 2H2O (l) → 2KOH (aq) + H2 (g) (c) 2HCl (g) + Mg (s) → MgCl2 (aq) + H2 (g) (d) 2P (s) + 5Cl2 (aq) → 2PCl5 (s) (e) 2Li (s) + Cu2+ (aq) → 2Li+ (aq) + Cu (s)

All of the reactions shown are oxidationreduction reactions except A) N2(g) + O2 (g) → 2...

All of the reactions shown are oxidationreduction reactions except A) N2(g) + O2 (g) → 2 NO(g) B) 2 Fe2O3 (s) → 4 Fe(s) + 3 O2 (g) C) Zn(s) + 2 HCl(aq) → ZnCl2 (aq) + H2 (g) D) CH4(g) + 2 O2 (g) → CO2(g) + 2 H2O(l) E) K2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2 KCl(aq)

Apply the half-reaction method to balance the following redox reactions 1. O2 + I- → I2 (in...

Apply the half-reaction method to balance the following redox reactions 1. O2 + I- → I2 (in base) 2. HNO3 + Bi2S3 → Bi(NO3)3 + NO + S (in acid) 3. SCN- + H2O2 → NH4+ + HCO3- + HSO4- (in acid)

Consider the five balanced chemical reactions listed below, all using O2 as a reactant. Normally, O2...

Consider the five balanced chemical reactions listed below, all using O2 as a reactant. Normally, O2 is an excess reagent for reactions because there is a large amount of it available in the air. For this question, suppose that you have5.73 moles of O2 and1.70 moles of any of the other reactants in every equation. Select those equations below in which O2 would be the limiting reactant. A.C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(g)B.C3H8(g) + 5 O2(g)...

Use the following half-reactions to write three spontaneous reactions, and calculate E cell for each reaction:...

Use the following half-reactions to write three spontaneous reactions, and calculate E cell for each reaction: a. Au+ (aq) + e- ----> Au (s) E= 1.69 V b. N2O (g) + 2H+ (aq) + 2 e- ----> N2 (g) + H2O (l) E= 1.77 V c. Cr3+ (aq) + 3e- ---> Cr (s) E= -0.74 V