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Mitchtwitchita
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Is there anybody that can tell me if I'm doing this question right?
Metallic Ca reacts with hydrochloric acid according to the following equation:
Ca(s) + 2 HCl(aq) ---> 2 CaCl2 (aq) + H2(g)
The enthalpy change associated with this reaction can be determined with an ice calorimeter. If 13.59 g of ice are melted when 0.3487 g of Ca reacts with excess hydrochloric acid, what is deltaH (in kJ/mol Ca) for the reaction written above? The heat of fusion of ice is 333 J/g.
qrxn + qfusion = 0
qrxn = ndeltaHrxn
=(13.59 g H2O)(0.333 kJ/g)
=4.53 kJ
0.3487 g Ca X 1 mol Ca/40.08 g Ca = 8.70 x 10^-3 mol
4.53 KJ/8.70 x 10^-3 mol = 521 kJ/mol?
Does this look right?
Metallic Ca reacts with hydrochloric acid according to the following equation:
Ca(s) + 2 HCl(aq) ---> 2 CaCl2 (aq) + H2(g)
The enthalpy change associated with this reaction can be determined with an ice calorimeter. If 13.59 g of ice are melted when 0.3487 g of Ca reacts with excess hydrochloric acid, what is deltaH (in kJ/mol Ca) for the reaction written above? The heat of fusion of ice is 333 J/g.
qrxn + qfusion = 0
qrxn = ndeltaHrxn
=(13.59 g H2O)(0.333 kJ/g)
=4.53 kJ
0.3487 g Ca X 1 mol Ca/40.08 g Ca = 8.70 x 10^-3 mol
4.53 KJ/8.70 x 10^-3 mol = 521 kJ/mol?
Does this look right?