Calculate the heat energy needed to heat 3.00moles of liquidwater from 50. o C t

Question

Calculate the heat energy needed to heat 3.00moles of liquidwater from 50.oC to 100.oC and boil itaway. The molar heat of fusion is 6.02kJ/mol, The molar heat of vaporization is 40.6kJ/mol, and Sice=2.09J/g deg C Sliquid=4.184J/gdegC Sgas=2.03J/g deg C A. 133kJ         B.11.3kJ          C.50.0kJ          D.122kJ           E. 1.14x104 kJ Calculate the heat energy needed to heat 3.00moles of liquidwater from 50.oC to 100.oC and boil itaway. The molar heat of fusion is 6.02kJ/mol, The molar heat of vaporization is 40.6kJ/mol, and Sice=2.09J/g deg C Sliquid=4.184J/gdegC Sgas=2.03J/g deg C A. 133kJ         B.11.3kJ          C.50.0kJ          D.122kJ           E. 1.14x104 kJ

Explanation / Answer

No . of moles of water , n = 3 mol No . of moles , n = mass / Molar mass Molar mass of water , H2O is = 2 * 1 + 16 = 18 g So mass of water , m = 3 mol * 18 g / mol = 54 g Quantity of heat required , Q = mcdt + mL where c = specific heat of water = 4.186 J / g oC         dt = change intemperature = 100 - 50 = 50 oC         L = Latent heat ofvapourization of water = 2260 J / g Plug the values we get Q = 54 * 4.186 * 50 + ( 54* 2260 )                                      = 133342.2 J                                      = 133.3422 KJ                                       ~ 133 KJ

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