Asked by Katherine
A generic solid, X, has a molar mass of 77.7 g/mol. In a constant-pressure calorimeter, 31.2 g of X is dissolved in 289 g of water at 23.00 °C.
The temperature of the resulting solution rises to 24.40 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there\'s negligible heat loss to the surroundings. How much heat was absorbed by the solution?
How much heat was absorbed by the solution?
The temperature of the resulting solution rises to 24.40 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there\'s negligible heat loss to the surroundings. How much heat was absorbed by the solution?
How much heat was absorbed by the solution?
Answers
Answered by
DrBob222
q = mass H2O X specific heat H2O x (Tfinal-Tinitial)
All the rest of that info is not needed UNLESS you want delta H/g and/or delta H/mol.
dH/g = q/31.2
dH/mol = q/g x (77.7 g/mol) = ?
All the rest of that info is not needed UNLESS you want delta H/g and/or delta H/mol.
dH/g = q/31.2
dH/mol = q/g x (77.7 g/mol) = ?
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