Using the data provided, what is the ΔH°rxn, in kJ/mol, for the equation below?   CO2(g) + 2CH4(g) ® C3H8(g) + O2(g)     Substance         ΔH°f (kJ/mol) CO2(g)              -393.5 CH4(g).             -74.9 C3H8(g)            -104.7   a) -438.6 kJ/mol b) 438.6 kJ/mol c) 363.7 kJ/mol d) 139.0 kJ/mol e) -363.7 kJ/mol

Given the data in the table below, determine ΔH°rxnfor the reaction             4NO (g)  +  6 H2O (l) →  4NH3 (g)  +  5 O2 (g)

2 NO(g) + O2(g) ––––> 2 NO2(g); ∆H° = –114.4 kJ Given the thermochemical equation above, how much heat is given off by the system when 951.1 g of NO2 is produced? (the molar mass of NO2 is 46.00 g/mol) A) 114.4 kJ B) 1.183 x 103 kJ C) 2.365 x 103 kJ D) 5.534 kJ E) 1.088 x 105 kJ

Given the following thermochemical equations, find ΔH° for the following reaction: 2NH3(g) + 2O2(g) ⟶ N2O(g) + 3H2O(l)                               ΔH˚ = ?   2NH3(g) + 4SO3(g) ⟶ N2O(g) + 4SO2(g) + 3H2O(l)            ΔH˚ = -290 kJ 2SO3(g) ⟶ 2SO2(g) + O2(g)                                                  ΔH˚ = 197 kJ

Given the following data: N2(g) + O2(g) → 2NO(g) ΔH = +180.6 kJ 2CO2(g) + N2(g) → 2CO(g) + 2NO(g) ΔH = 746.6 kJ Find the ΔH of the following reaction: 2CO2(g) → 2CO(g) + O2(g)

what is the value of ΔHrxn if the reaction below is reversed? In other words, PCl5 becomes the reactant. Report your answer in kJ to 1 decimal place. PCl3(g) + Cl2(g) → PCl5(g); ΔHrxn = 618.7 kJ

Calculate ΔH°rxn for the reaction 2Ni(s)+2S(s)+3O2​(g)2NiSO3​(s)  from the following information: 1. NiSO3​(s)NiO(s)+SO2​(g) ΔHorxn​=156 kJ 2. S(s)+O2​(g)SO2​(g)              ΔHorxn​=−297 kj 3. Ni(s)+1/2​O2​(g)NiO(s) ΔHorxn​=−241 kJ

Titanium(IV) oxide is commonly used as a white paint pigment. The compound is produced by the reaction TiCl 4(g) + 2 H 2O(g)↔ TiO 2(s) + 4 HCl(g) What is ΔH° rxn (in kilojoules)? TiCl 4(g) ΔH f o = -763 kJ/molH 2O(g) ΔH f o = -241.8 kJ/mol.HCl(g) ΔH f o = -92 kJ/mol.TiO 2(s) ΔH f o = -945 kJ/mol.

Suppose 9.44 g of calcium chloride, CaCl2, (MM=111.0 g/mol) is added to 222. g water at 21.84oC in a styrofoam cup calorimeter, and the temperature rose to 29.76oC.  Calculate a value for ΔH  in the equation:  CaCl2(s) + H2O(l) → Ca2+(aq) + 2Cl-(aq)    ΔH = ??? kJ/mol. (Assume that the styrofoam cup does not absorb any heat nor allow any heat loss; assume the specific heat of the resulting solution is 3.88 J/(goC))

A calorimeter contains 16.0 mLmL of water at 12.5 ∘C∘C . When 1.40 gg of XX (a substance with a molar mass of 75.0 g/molg/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq)X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C∘C . Calculate the enthalpy change, ΔHΔ�, for this reaction per mole of XX. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)J/(g⋅∘C)],  that density of water is 1.00 g/mLg/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures.