Calculate the enthalpy of formation of methanolweb.whrhs.org/webfiles/mamendola/Chem H/2009_2010...
Transcript of Calculate the enthalpy of formation of methanolweb.whrhs.org/webfiles/mamendola/Chem H/2009_2010...
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Given the following heats of combustion. CH3OH(l) + 3/2 O2(g) CO2(g) + 2 H2O(l) ΔH°rxn = 726.4 kJ
C(graphite) + O2(g) CO2(g) ΔH°rxn = 393.5 kJ
H2(g) + 1/2 O2(g) H2O(l) ΔH°rxn = 285.8 kJ
Calculate the enthalpy of formation of methanol (CH3OH) from its elements. C(graphite) + 2 H2(g) + 1/2 O2(g) CH3OH(l)
What is the equation for the enthalpy of formation of sodium hypochlorite?
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A quantity of 2.00 x 102 mL of 0.862 M HCl is mixed with 2.003 x 102 mL of 0.431 M Ba(OH)2 in a constantpressure calorimeter that has a heat capacity of 453 J/°C. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.48°C. For the following process the heat of neutralization is 56.2 kJ. H+(aq) + OH(aq) H2O(l)What is the final temperature of the mixed solution?
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From the data shown below, calculate the enthalpy change for the following transformation. S(rhombic) S(monoclinic)(Monoclinic and rhombic are different allotropic forms of elemental sulfur.) S(rhombic) + O2(g) SO2(g) ΔH°rxn = 296.06 kJS(monoclinic) + O2(g) SO2(g) ΔH°rxn = 296.36 kJ
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Calculate the heat of decomposition for this process at constant pressure and 25°C. (Look up the standard enthalpy of formation of the reactant and products in Table 6.4 and appendix; ΔH°f(BaCO3(s)) = 1218.8 kJ/mol, ΔHf (BaO(s)) = 558.2 kJ/mol and ΔH°f (Na2CO3(s)) = 1130.9 kJ/mol, ΔH°f (Na2O(s)) = 415.89 kJ/mol.)1 kJ CaCO3(s) CaO(s) + CO2(g)
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A sheet of gold weighing 10.0 g and at a temperature of 18.0°C is placed flat on a sheet of iron weighing 20.0 g and at a temperature of 55.6°C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. (Hint: The heat gained by the gold must be equal to the heat lost by the iron.)
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Methanol (CH3OH) is an organic solvent and is also used as a fuel in some automobile engines. From the following data, calculate the standard enthalpy of formation of methanol. 2 CH3OH(l) + 3 O2(g) 2 CO2(g) + 4 H2O(l) ΔH°rxn = 1452.8 kJ
2 CH3OH(l) + 3 O2(g) 2 CO2(g) + 4 H2O(l) ΔH°rxn = 1452.8 kJ
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The values of the two allotropes of oxygen, O2 and O3, are 0 and 142.2 kJ/mol, respectively, at 25°C. Which is the more stable form at this temperature?