Part C Add the following reactions together: ClO(g)+O3(g)ClO2(g)+O(g)??ClO2(g)+O2(g)ClO(g)+O2(g) Identify which species are intermediates, which are catalysts,...

Part C

Add the following reactions together:

ClO(g)+O3(g)ClO2(g)+O(g)??ClO2(g)+O2(g)ClO(g)+O2(g)

Identify which species are intermediates, which are catalysts, and which are only reagents or products.

Drag each item to the appropriate bin.

SubmitHintsMy AnswersGive UpReview Part

Expert Solution

Following are the given reactions 1 and 2:

ClO (g) + O₃ (g) -------------> ClO₂ (g) + O₂ (g)……………reaction1

ClO₂ (g) + O(g) ----------------> ClO (g) + O₂ (g)……………reaction2

____________________________________________________________

Add them: ClO (g) + O₃ (g) + O(g) ------> 2O₂ (g) + ClO (g)……….net reaction

ClO₂ is an intermediate as it is generated in the reaction 1 and consumed in reaction 2. As can be seen from the net reaction no ClO₂ appears in it.

ClO is a catalyst as it has reacted in the reaction 1 but regenerated in the reaction 2.

O₃ and O are reactants and O2 is the product.

queen_honey_blossom answered 12 hours 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 ΔrH for the following reaction: C(s)+H2O(g)→CO(g)+H2(g) Use the following reactions and given ΔrH's. C(s)+O2(g)→CO2(g), ΔrH=...

Calculate ΔrH for the following reaction: C(s)+H2O(g)→CO(g)+H2(g) Use the following reactions and given ΔrH's. C(s)+O2(g)→CO2(g), ΔrH= -393.5 kJmol−1 2CO(g)+O2(g)→2CO2(g), ΔrH= -566.0 kJmol−1 2H2(g)+O2(g)→2H2O(g), ΔrH= -483.6 kJmol−1 Express your answer using one decimal place.

Which of the following reactions is spontaneous as written? C(s) + 2H2 (g) = CH4 (g)...

Which of the following reactions is spontaneous as written? C(s) + 2H2 (g) = CH4 (g) 2H2 (g) + O2 (g) = 2H2O(l) 4HCN(g) + 5O2(g) = 2H2O(l) + 4CO2(g) 2N2(g) NaI(s) = Na+(aq) + I-(aq)

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.

1)Using average bond enthalpies, predict which of the following reactions will be most exothermic: a) C(g)...

1)Using average bond enthalpies, predict which of the following reactions will be most exothermic: a) C(g) + 2 F2(g) b) CO(g) +3 F2(g) CF4(g) + OF2(g) c) CO2(g) + 4 F2(g) CF4(g) + 2 OF2(g) 2) Ammonia is produced directly from nitrogen and hydrogen. The chemical reaction is N2(g) + 3 H2(g) 2 NH3(g) N≡N a) Use Table 8.4 p 326 in textbook (or you can find the table in the chapter 5 slides on the UR course), to estimate...

Exercise 18.62 Calculate E∘cell for each of the following balanced redox reactions. Part A O2(g)+2H2O(l)+4Ag(s)→4OH−(aq)+4Ag+(aq) Express your answer...

Exercise 18.62 Calculate E∘cell for each of the following balanced redox reactions. Part A O2(g)+2H2O(l)+4Ag(s)→4OH−(aq)+4Ag+(aq) Express your answer using two significant figures. E∘cell = V Part B Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express your answer using two significant figures. E∘cell = V Part C PbO2(s)+4H+(aq)+Sn(s)→Pb2+(aq)+2H2O(l)+Sn2+(aq) E∘cell = v

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)...

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq) D. Determine whether the reaction in part A is spontaneous as written. E. Determine whether the reaction in part B is spontaneous as written. F. Determine whether the reaction in part C is spontaneous as written.

Question