Which one of the following reactions, when carried out at 25 °C and 101.3 kPa pressure, has an enthalpy change corresponding to the standard molar enthalpy of formation, ∆Hf°, of C2H5OH (l) ?
E. 2 C (s) + 3 H2 (g) + 1/2 O2 (g) → C2H5OH (l)
Which one of the following reactions, when carried out at 25 °C and 101.3 kPa pressure,...
Use the Data table to calculate ∆H for the reaction below:Reactions: Change in Enthalpy (∆H)(1) C (s) + O2 (g) -> CO2(g) ∆H1 = -393.5 kJ/ mol(2) H2 (g) + 1/2 O2 (g) -> H2O (l) ∆H2 = -285.8 kJ/mol(3) 2C2H6 (g) + 7O2 (g) -> 4 CO2 (g) + 6 H2O (l) ∆H3 = -283.0 kJ/molCalculate the enthalpy change for the reaction:2 C (s) + 3 H2 (g) -> C2H6(g) ∆H = ______________kJ/mol
Calculate the change in enthalpy (ΔH) for the heat of formation of ethane, C2H6, using Hess' Law and the following reactions:a) 2C(S) + 2O2(g) → 2CO2(g), ΔH = -188 kcalb) C2H6(g) + (7/2)O2(g) → 2CO2(g) + 3H2O(l), ΔH = -373 kcalc) H2(g) + (1/2)O2(g) → H2O(l), ΔH = -68.3 kcal
Using Thermodynamic Data (∆Hf), calculate the enthalpy change (∆Hrxn) for the following reactions: Fe2O3 (s) + H2 (g) → Fe (s) + H2O (l) N2H3CH3 (l) + N2O4 (l) → H2O (g) + N2 (g) + CO2 (g) C6H12O6 (s) + O2 (g) → CO2 (g) + H2O (g)
Enthalpy changes for the following reactions can be determined experimentally: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l) C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) ΔHorxn = -1411.1 kJ/mol-rxn ΔHorxn = -1367.5 kJ/mol-rxn Use the given values to determine the enthalpy change for the reaction: C2H4(g) + H2O(l) → C2H5OH(l) ΔHorxn (answer) = kJ/mol-rxn
Use the enthalpies for the given reactions to compute the standard enthalpy change (ΔH°) for the reaction: 6 C (s) + 7 H2(g) → C6H14 (l) ΔHrxn = ? C6H14 (l)+19/2O2 (g)→6CO2(g)+ 7H2O(g). ΔH=–3505.8kJ C(s) + O2 (g) → CO2(g) ΔH=–393.5kJ H2(g) + 1/2 O2(g) → H2O(g). ΔH = – 242.0 kJ
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol ______kJ/mol
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
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, Δ H o f CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol
A.A scientist measures the standard enthalpy change for the following reaction to be -2932.6 kJ : 2C2H6(g) + 7 O2(g)4CO2(g) + 6 H2O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO2(g) is kJ/mol. B.A scientist measures the standard enthalpy change for the following reaction to be -138.9 kJ : H2(g) + C2H4(g)C2H6(g) Based on this value and the standard enthalpies of formation for the other substances, the standard...
Which one of the following is not a state function ? change in temperature internal energy enthalpy heat Calculate ΔH for the following reaction C2H4 (g) + 6 F2 → 2 CF4 (g) + 4 HF (g) from H2 (g ) + F2 (g) → 2 HF (g) ΔH = - 537 kJ C (s) + 2 F2 (g) → CF4 (g) ΔH = -680 kJ 2 C (g) + 2 H2 (g) → C2H4 (g) ΔH = + 52 kJ...