Calorimetry Problem: Calculate Final Temp.

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To calculate the final temperature of a solution when dissolving 25.00g of AgNO3 in 250.0mL of water at an initial temperature of 21.75°C, the heat from the dissolution reaction must be considered. The enthalpy change (ΔH) of 0.908 kJ indicates the heat absorbed during the process. The heat capacity of the solution can be assumed to be that of pure water, while the calorimeter's heat capacity must also be included in the calculations. The total heat absorbed by both the solution and the calorimeter will determine the final temperature. Accurate calculations will require converting the enthalpy value to J/mol and using the mass of the final solution along with the heat capacity values.
Acidburn
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I have a question that i cannot get an answer too.

AgNO3 (s) ---> Ag (aq) + NO3 (aq)

THESE ARE THE GIVEN:
ΔH=0.908 kJ
c(Cu)=0.3900 J/g ͦC
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Calculate the final temperature of a solution if 25.00g of pure AgNO3 is dissolved in 250.0mL of water (initially at 21.75 ͦC) in a 750.0g copper calorimeter.

Answers are appreciated. Thanks!
 
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You are to assume that the solution water heat capacity is that of pure water. Other than that you have one source of heat and heat is absorbed by both copper calorimeter and solution.

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yeah thermochem was always hell. i think you need to find the amount of heat from the reaction. is that enthalpy value J/mol? well, you know how many moles are reacting (simple conversion). you also know the mass of the final solution and as was stated in the previous post, you have heat capacity values.
 

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