Elemental sulfur occurs in several forms, with rhombic sulfur the most stable under normal conditions and monoclinic sulfur somewhat less Calculate the change in enthalpy for the rhombic to monoclinic transition as shown by the following reaction: S(s, rhom) → S(s, mono) S(s, rhom)  + O2(g) → SO2(g)               ΔH  =  −296.83 kJ S(s, mono) + O2(g) → SO2(g)             ΔH = −297.16 kJ

The synthesis of Hansa yellow dye takes place in a series of two steps. On Sunday June 9th, 1996 a violent runaway reaction occurred causing very significant damage to equipment and buildings. After a detailed analysis, the plant was rebuilt, and production resumed. What is the enthalpy of the overall reaction? Show work for credit. Can you explain which of the two steps was most likely to blame for the incident? Step 1: CsH;CIN2O2(aq) + NANO2(aq) + 2HCI(aq) → C6H3CIN3O2*(aq) + Cl(aq) + 2H2O(I) + NaCI(aq) AH1 = -1212 kJ/mol Step 2: C6H3CIN3O2*(aq) + Cl'(aq) + C10H10CINO2(aq) → C16H12C12N4O4(aq) + HCl(aq) AH2 = 637 kJ/mol %3| Overall Reaction: C6H5CIN2O2(aq) + NaNO2(aq) + HCI(aq) → 2H2O(1) + NaCI(aq) + C16H12CI2N4O4(aq) AHrxn = ? kJ/mol %3D

(D 263 kJ/mol P. 22. Using the following thermochemical equations: C(s) + O,(g) → CO,(g) ΔΗΟ. rxn 1 =-394 kJ/mol,Txn C(s) + CO,(g) → 2 CO(g) AH°. Ixn 2 =+173 kJ/mol,xa Determine the enthalpy of the reaction represented below: 2 C(s) + 0,(g) → 2 CO(g) ΔΗ Txn 3 = ? 1> (A) ΔΗ. :-567 kJ/molxn rxn (В) ДН =-221 kJ/mol,xn (С) ДН =+221 kJ/molpxn (D) AH°. +567 kJ/molpxn %3D Ixn qt ian od geind hw qua boalunai na cop d ofiosa orb d A 100--32 HO0-02 X convinn or rmrainn an nart of this nanA iR llanal.

An ammonia refrigeration cycle involves the conversion of 0.56 kg of liquid ammonia into vapor every minute at the boiling-point temperature. At what rate does the ammonia absorb energy?

Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as losing heat to the surroundings? q=-, w = - q=+, W = + q=, W = + q=+, w = - O None of these represent the system referenced above.

Given the following thermochemical equations: 4 FeS2(s) + 11 O2(g) 2 H2S(g) + 3 O2(g) → 2 Fe2O3(s) + 8SO2(g) → 2 H₂O(1) +2 SO2(g) →2 Fe2O3(s) 4 FeO(s) + O2(g) →2 FeO(s) 2 Fe(s) + O2(g) H2(g) +S(s) 2 H2(g) + O2(g) → H₂S(g) → 2 H₂O(1) Compute the AH for FeS2(s) in kJ/mol. A)-1233.9 kJ/mol B) -2893.9 kJ/mol C) -24.3 kJ/mol D) -183.5 kJ/mol E) -70.0 kJ/mol O A OB Oc OD OE (kJ/mol) ΔH° = -3307.9 - 1125.2 -578.2 -544 - 20.2 -571.7

Fluorine (F2), the most electronegative element reacts with water in a different way compared to other halogens do. With excess water, fluorine reacts with water to produce hydrofluoric acid and oxygen gas in the following reaction: 2F2(g) + 2H2O() →4HF (1) + O2(g) Calculate AHrxn for the process above from the following information: AH= +571.6 kJ (a) AH= +542.0 kJ (b) 2H₂O(1)→ 2H2(g) + O2(g) 2HF (g) → H2(g) + F2(g) Which equation(s) will you flip? O a. Only equation (b) O b. Only equation (a) O c. Both equations will be flipped. O d. No equations will be flipped.

Using the information provided along with an understanding of Hess's Law, determine the enthalpy of reaction for the unknown reaction. AFels) + 3Sn0,(s) → 2Fe,0,(s) +3Sn(s) 2Fe(s) +0, (s) - Fe;0,(s) A,H = -824.2 k) Sn{s) + 0,(g) - Sn02(s) AyH=-580.7 k/

The steps of the Born-Haber cycle are shown for the ionic compound MX2, made up of generic metal M and generic, gaseous halogen X. Identify the overall reaction and identify the name of the enthalpy change for each reaction.