A 50.0-mL sample of 0.400 M copper(II) sulfate solution at 23.35 °C is mixed with 50.00 mL
of 0.600 M sodium hydroxide solution, also at 23.35 °C, in the coffee-cup calorimeter. After
the reaction occurs, the temperature of the resulting mixture is measured to be 25.23 °C.
The density of the final solution is 1.02 g/mL. Calculate the amount of heat evolved.
Assume that the specific heat of the solution is the same as that of pure water, 4.184 J/g·°C.
The heat capacity of the calorimeter is 24.0 J/°C.
CuSO4(aq) + 2NaOH(aq) → Cu(OH)2(s) + Na2SO4(aq)

Question

A 50.0-mL sample of 0.400 M copper(II) sulfate solution at 23.35 °C is mixed with 50.00 mL 
of 0.600 M sodium hydroxide solution, also at 23.35 °C, in the coffee-cup calorimeter. After 
the reaction occurs, the temperature of the resulting mixture is measured to be 25.23 °C. 
The density of the final solution is 1.02 g/mL. Calculate the amount of heat evolved. 
Assume that the specific heat of the solution is the same as that of pure water, 4.184 J/g·°C. 
The heat capacity of the calorimeter is 24.0 J/°C. 
 CuSO4(aq) + 2NaOH(aq) → Cu(OH)2(s) + Na2SO4(aq)

aaronq · Answer

the heat evolved from the reaction is distributed into both the calorimeter and the solution.

$q_{total}=q_{water}+q_{calorimeter}$


$=m_{water}*C_p*(T^{mixture}_f-T^{solution}_i)+C^{cal}_p*(T^{mixture}_f-T^{cal}_i)$



$=-\underbrace{(100mL*1.02 g/mL)}*(4.184 J/g·°C)*(25.23-23.35 °C)+.. $
                       m=$\rho$*V


you can fill in the rest after the plus sign

aaronq · Answer

because it's too long and wont fit

aaronq · Answer

wait ignore the (-) minus sign in the last equation

aaronq · Answer

this one is different look at it http://openstudy.com/study#/updates/52f2e8cce4b0d693ffe47a72