Given C2H6 (g) ---> 3H2 DeltaH: 84.7 KJ
Give the enthalpy for 4x reverse reaction and for making 556 grams of H2 product. (two part problem)
A) enthalpy for 4 × reverse reaction
∆H° = -4×84.7 => -338.8 kJ
B) enthalpy for making 6 g H2 = 84.7 kJ
Enthalpy for making 556 g H2 = 84.7×556/6.0
∆H = 7848.9 kJ
Given C2H6 (g) ---> 3H2 DeltaH: 84.7 KJ Give the enthalpy for 4x reverse reaction and...
For the reaction: H2(g)+C2H4(g)-->C2H6(g) Bond & Bond Enthalpy H-H 436.4 kJ/mole C-H 414 kJ/mol C-C 347 kJ/mol C=C 620 kJ/mol Substance & delta Hf H2 0 C2H4 52.3 C2H6 -84.7 (a) estimate the enthalpy of reaction, using the bond enthalpy values from the table in kJ/mol (b) Calculate the enthalpy of reaction, using standard enthalpies of formation
problem is together.
3. Calculate the enthalpy of formation of carbon dioxide in the following reaction: C(s) + O2(g) - CO, (g) Use the following equations: a) H2O(l) → H2(g) + 2O2(g) AH°-= +285.8 kJ/mol b) C2H6(g) → 2C (s) + 3H2(g) AH'= +84.7 kJ/mol c) 2CO2 (g) +3H2O (1) C2H6(g) + (7/2) O2(g) AH°F = +1560.7 kJ/mol
Estimate the enthalpy change for the following reaction : H2(g) + C2H4(g) -------> C2H6(g), given the following bond energies: BE(H-H) = 436 kJ/mol; BE(C-H) = 414 kJ/mol; BE(C-C) = 347 kJ/mol; BE(C=C) = 620 kJ/mol. A. -119 kJ B. +119 kJ C. -392 kJ D. +392 kJ E. none of the above
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
What is the enthalpy of the following reaction: CH4(g) + NH3(g) à HCN(g) + 3H2(g) Use the data from the following three reactions: N2(g) + 3H2(g) à 2NH3(g) DrH° = -91.8 kJ C(s) + 2H2(g) à CH4(g) DrH° = -74.9 kJ H2(g) + 2C(s) + N2(g) à 2HCN(g) DrH° = +270.3 kJ 437 kJ 150 kJ 391 kJ 287 kJ 256 kJ
1. For the reaction H2S(g) + 2H2O(l)3H2(g) + SO2(g) H° = 295.4 kJ and S° = 294.7 J/K The equilibrium constant for this reaction at 345.0 K is _____ Assume that H° and S° are independent of temperature. 2. For the reaction H2+ C2H4 -> C2H6 H° = -137.0 kJ and S° = -120.7 J/K The equilibrium constant for this reaction at 264.0 K is ______. Assume that H° and S° are independent of temperature
for the chemical reaction H2(g) + F2(g) → 2HF(g); ∆H°=-79.2 kj/mol what is the enthalpy for the reaction 3H2+3F2->6HF
Given the following thermochemical data, what is the standard enthalpy of combustion of C2H6 in kJ·mol–1? H2 (g) + 1/2 O2 (g) → H2O (l) ΔH0= –286 kJ C2H4 (g) + H2 (g) → C2H6 (g) ΔH0= –137 kJ C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (l) ΔH0= –1412 kJ
1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) + 3.5O2 (g) -----> 2CO2 (g) + 3H2O (l) ΔH2 = -1560 kJ/mo 3) C2H4 (g) + 3O2 (g) -----> 2CO2 (g) + 2H2O (l) ΔH3 = -1411 kJ/mol 4) 2H2O (l) -----> 2H2 (g) + O2 (g) ΔH4 = 571.6 kJ/mol How much heat is transferred between the system and the surroundings when 25 grams of ethane (C2H6) decomposes to produce ethylene (C2H4) and...
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 20 °C given that ∆rG° = -92.2 kJ mol-1, P(C2H4) = 1.41×10-2 bar, P(H2) = 1.47×10-2 bar, and P(C2H6) = 3.00×10-1 bar.