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Mg (s) + ½O 2(g) → MgO (s) D H= _____

key. Names: ___________________________________. All encompassing activity…A.P. Chemistry Ch. 6. -626 kJ. Mg (s) + ½O 2(g) → MgO (s) D H= _____. MgO (s) + 2HCl (aq) → MgCl 2(aq) + H 2 O (l) D H = _______. -100 kJ. flipped. Add these steps:.

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Mg (s) + ½O 2(g) → MgO (s) D H= _____

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  1. key Names: ___________________________________ All encompassing activity…A.P. Chemistry Ch. 6 -626 kJ Mg(s) + ½O2(g) → MgO(s)DH= _____ MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) DH = _______ -100 kJ flipped Add these steps: Mass of MgO = 0.50 g (0.013 mol)←L.R. Volume of HCl = 50.0 mL (3.0 M) DT = 6.3° C (typical temperature change with the amounts used) qwater = (50.0 g)(4.184 J/g°C)(6.3°C) = 1318 J qsys = -1318 J DHrxn= -1318 J/ 0.013mol = -1.0 x 105 J/mol 100 kJ MgCl2(aq) + H2O(l) → MgO(s) + 2HCl(aq)DH = Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)DH = -440 kJ -286 kJ H2(g) + ½O2(g) → H2O(l)DH= Mg(s) + ½O2(g) → MgO(s)DH= _____ -626 kJ Of Note: the accepted value for the heat of formation of MgO is -602kJ…if you don’t believe me look it it up H2(g) + ½O2(g) → H2O(l)DH= _____ -286 kJ Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) DH = _______ -440 kJ Mass of Mg = 0.50 g (0.021 mol)←L.R. Volume of HCl = 50.0 mL (3.0 M) DT = 44.2° C (typical temperature change with the amount that used) qwater= (50.0 g)(4.184 J/g°C)(44.2°C) = 9240 J qsys= -9240 DHrxn= -9240 J/ 0.021mol = -440,000 J/mol

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