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Solution: During an experiment, a student adds 1.23 g of CaO to 200.0 mL of 0.500 M HCI. The student observes a temperature increase of 5.10°C. Assuming the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/(g.°C), calculate the heat of the reaction (kJ/mol), ΔHrxn.CaO (s) + 2H+ (aq) → Ca2+ (aq) + H2O (l) 

Problem

During an experiment, a student adds 1.23 g of CaO to 200.0 mL of 0.500 M HCI. The student observes a temperature increase of 5.10°C. 

Assuming the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/(g.°C), calculate the heat of the reaction (kJ/mol), ΔHrxn.

CaO (s) + 2H+ (aq) → Ca2+ (aq) + H2O (l) 



Solution

We can calculate the enthalpy of reaction using the equation below :

Here q is the heat absorbed by the solution and n is the number of moles reacted. 

Now we have to find out first the limiting reactant in this reaction.

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