∆Hrxn
= ∆Hf (CH3CH2OH) + ∆Hf (H2O) - ∆Hf (C2H5OH) - ∆Hf (O2)
= -484.5 + (-285.8) - (-277.7) - (0)
= -492.6 kJ
4. Given the following standard enthalpy of formations: AH° C,H,OH() =-277.7 kJ/mol]; AHO [CH CO H) = 484.5 kJ/mol]...
Given the following standard enthalpy of formations: AH [C,H,OH() --277.7 kJ/mol; AH(CH3CO,H() = -484.5 kJ/mol); AH® [H2O(1) --285.8 kJ/mol]; AH [O2(g) - 0 kJ/mol). Calculate the AHan for the reaction. C,H,OH(I)+,(g) → CH,CO,H(1) + H2O(l)
6. Given the following thermochemical reactions 2NO N,+O 2NO+O,2NO AH=-180 kJ AH=-112 kJ Calculate the enthalpy change of the reaction of nitrogen with oxygen to produce nitrogen dioxide. N,+20,2NO, AH r? Lo Given the following standard enthalpy of formations: AHor [C2H$OH(I) =-277.7 kJ/mol]; AHOr [CHCO2H) =-484.5 kJ/mol]; AHr [H2O) = -285.8 kJ/mol]; AHn[O2(g) = 0 kJ/mol]. Calculate the AHn for the reaction. C,H.OH()+O,(g) ->CH,CO,H() + H2O(1)
3. Mothballs are composed primarily of the hydrocarbon naphthalene (C,H). When 1.25 g naphthalene is burned in a bomb calorimeter, the temperature rises from 25.25 °C to 34.33 °C. (Heat capacity of calorimeter 5.11 kJ/°C). Calculate: a) The heat of reaction per gram of naphthalene b) The heat of reaction per mole of naphthalene Given the following standard enthalpy of formations: AH°, [C,H,OHO --277.7 kJ/mol]; AH [CHCOH) = 484.5 kJ/mol]; AH [HO) = -285.8 kJ/mol]; AH® [0,(g) - 0 kJ/mol].
Calculate the standard enthalpy of formation of CS2() given that AH=-393.5 kJ/mol AHo = -296.4 kj/mol a. C(s) + O2(g) CO2lg) b. S(s) +O2(g). SO2(g) AH = -1073.6 kj/mol C. CS2(I)+302(g) Co2lg) + 2S02(B)
ate the standard enthalpy change for the reaction Given standard enthalpy of formations △H; (SO(g))--395.2 kJ/mol Δ} l; (SO2(g))--296.9 kJ/mol al 201.0 kJ 403 J 254.6 kJ - 120.4 k.J - 196.6 kJ dl
3. You are given the following standard enthalpies of formation at 25°C. HF (aq) -320.1 kJ/mol OH(aq) -230.0 kJ/mol F (aq) -332.6 kJ/mol H:0 (1) -285.8 kJ/mol a. Calculate the standard enthalpy of neutralization of HF (aq) HF (aq) + OH(aq) F (aq) + H20 (1) b. Using the value of -56.2 kJ/mol as the standard enthalpy change for the reaction H' (aq) + OH(aq) - H20 (1) calculate the standard enthalpy change for the reaction HF (aq) - H(aq)...
5. Calculate the enthalpy of formation of carbon dioxide in the following reaction: C(s) + O2(g) - CO. (g) 213 Use the following equations: 2) H.O (0) -- H() .O() AH: 285.8 kJ/mol b) CH. (g) -- 2C). 3H2(g) AH: +84.7 kJ/mol c) 200,(e) +3H.0 (6-- C.H. (B). (7/2)0,() AH - 1560.7 kJ/mol
Carbon monoxide can be formed by the reaction of carbon and steam AHo -352.3 kJ/mol C(s) +H2O(B) CO(B)Hz(g) Calculate the standard enthalpy of formation of CO(g) if the standard enthalpy of the reaction 02 (g) + 2H2(g) is AHo -483.6 kj/mol. 2 H20(g)
4. Use the bond enthalpies below and calculate the enthalpy of ethane combustion in kJ / mol. (AH° (H-H) = 436 kJ mol', AH° (C-H) = 435 kJ mol', AH° (0=0) = 498, AH° (CEO) = 732, AH (H-O) = 463] CzH6 (g) + 7/202 (g) - 2002 + 3H20 (g)
Question 4 of 4 > The enthalpy changes, AH, for three reactions are given. H, ()0,()H,O) Ca(s) +2H (aq) Ca2 (aq) +H,(g) CaO(s) +2H (aq) - AH=-286 kJ/mol AH= -544 kJ/mol Ca2 (aq) +H,O() AH =-193 kJ/mol Using Hess's law, calculate the heat of formation for CaO(s) using the reaction shown. 0,()Ca) Ca(s) + kJ/mol ΔΗ- TOOLS During an experiment, a student adds 1.81 g CaO to 300.0 mL of 1.000 M HCI. The student observès a temperature increase of...