Asked by Tyler
Assuming that the specific heat of the solution is 4.18 J/(g⋅∘C) and that the calorimeter itself absorbs a negligible amount of heat, calculate ΔH in kilojoules for the reaction
CaO(s)+H2O(l)→Ca(OH)2(aq)
When 1.045 g of CaO is added to 50.0 mL of water at 25.0 ∘C in a calorimeter, the temperature of the water increases to 32.3 ∘C.
CaO(s)+H2O(l)→Ca(OH)2(aq)
When 1.045 g of CaO is added to 50.0 mL of water at 25.0 ∘C in a calorimeter, the temperature of the water increases to 32.3 ∘C.
Answers
Answered by
DrBob222
dH for THIS reaction (just the 1.045g) is
q = 50g x 4.184 x (Tfinal-Tinitial).
MOST of the time these problems want the answer expressed in kJ/mol. If that is the case here that would
dH in kJ/mol = q from above x (molar mass CaO/1.05g) x (1 kJ/1000 J) = ? aprox 82 kJ/mol
q = 50g x 4.184 x (Tfinal-Tinitial).
MOST of the time these problems want the answer expressed in kJ/mol. If that is the case here that would
dH in kJ/mol = q from above x (molar mass CaO/1.05g) x (1 kJ/1000 J) = ? aprox 82 kJ/mol
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