Which reaction shows that the enthalpy of formation of C2H4 is Hf = 52.5 kJ/mol?A.2C(s) + 2H2(g) + 52.5 kJ C2H4B.2C(s) + 4H(g) C2H4 + 52.5 kJC.2C(s) + 2H2(g) C2H4 + 52.5 kJD.2C(s) + H(g) + 52.5 kJ C2H4SUBMITarrow_backPREVIOUS

Which reaction shows that the enthalpy of formation of CS2 is Hf = 89.4 kJ/mol?A.C(s) + 2S(s) + 89.4 kJ CS2(l)B.C(s) + 2S(s) + 89.4 kJ CS2(l) + 89.4 kJC.C(s) + 2S(s) CS2(l)D.C(s) + 2S(s) CS2(l) + 89.4 kJSUBMITarrow_backPREVIOUS

Using Hess’s Law, determine the enthalpy of reaction for,C2H4(g)   +  H2(g)   –>  C2H6(g)     ΔH = ?Using the following reactions:C2H4(g)   +   3O2(g)   –>  2CO2(g)   +  2H2O(l)  ΔH = -1401 kJC2H6(g)  +  7/2O2(g)   –>   2CO2(g)   +  3H2O(l)  ΔH = -1550 kJH2(g)  +    1/2O2(g)  –>  H2O(l)    ΔH = -286 kJGroup of answer choices243 kJ-311 kJ95 kJ-137 kJ

If enthalpies of formation of C2H4( g),CO2( g) and H2O(l) at 25∘C and 1 atm pressure are 52,394 and −286 kJ/mol respectively, the change in enthalpy for combustion of C2H4 is equal to

Given the following thermochemical data, what is the enthalpy of formation ΔfHo for C2H5OH(l) C(s)  +  O2(g)  →  CO2(g)                               ΔHo = –393 kJ mol–1H2(g)  +  1/2 O2(g)    →  H2O (g)                  ΔHo = -296 kJ mol–1C2H5OH +3O2 →  3H2O (g) + 2CO2(g)       ΔHo =–1369 kJ mol–1 Use-full formula ΔrxnHo=  ∑ ΔfHoproducts -  ∑ ΔfHoreactants

Which equation represents the reaction for which the enthalpy change, ∆H, is the meanbond enthalpy of the C–H bond?A ¼CH 4(g) → ¼C(g) + H(g)B CH 4(g) → C(s) + 2H 2 (g)C CH 4(g) → C(g) + 4H(g)D CH 4(g) → C(g) + 2H2 (g)