Name: Sebastian Sak Lab Partners: Tim Gronet
TA: Feifei Xu
Determining Molar Enthalpy of Dehydration of Sodium Acetate Trihydrate
Purpose:
In this lab, two solid substances, sodium acetate and sodium acetate trihydrate, will be analyzed for the heat of solution for both processes. This allowed the calculation of the molar enthalpy of dehydration of sodium acetate trihydrate. Calorimetry was used to experimentally determine the heat of solution for both reactions.
Procedure: This lab was performed based on the procedure outlined in “Exp #7 Calorimetry.” No changes to the procedure were made.
Data and Observations: All data and observations were recorded in the lab notebook. Pages from the lab notebook are attached to the lab.
Results …show more content…
The molar enthalpy of dehydration is not able to be determined in a one-step calorimetry experiment because the dissociation of ions occurs when the solution dissolves in water. Hess’s Law allows for the two thermochemical equations to be added resulting in a net equation, one that describes the molar enthalpy of dehydration. Calorimetry is using a tool, the calorimeter, which insulates the system from the environment. This allows for the changes of temperature to be observed with minimal heat loss to the environment. Calorimetry allows for the heat of the solution to be calculated since the heat capacity of the calorimeter is known and the change in temperature is observed. The heat capacity is the ability for the container to retain the heat the is produced or absorbed without allowing for the outside environment to impact the reaction. This closed system allows for easy calculations where q_rxn+q_water+q_calorimeter=0. This is important to the lab that the total heat lost and gained must all equal zero. It would be hard to calculate how much heat was lost in the world by the experiment, so isolating the system to the calorimeter allows for the …show more content…
This was confirmed by the values obtained from the Handbook of Chemistry and Physics. The experiment involved the use of calorimetry and Hess’s Law to calculate the molar enthalpy of dehydration. An important improvement to increase the accuracy of the data would be to use a digital thermometer with shorter intervals in recording the data, especially when the reaction is occurring. This would improve identifying the true final temperature of the system. Another improvement would be to use a calorimeter that better retains heat. This would also increase the accuracy of the final temperature that the solution obtains as less heat is lost to the
TA: Feifei Xu
Determining Molar Enthalpy of Dehydration of Sodium Acetate Trihydrate
Purpose:
In this lab, two solid substances, sodium acetate and sodium acetate trihydrate, will be analyzed for the heat of solution for both processes. This allowed the calculation of the molar enthalpy of dehydration of sodium acetate trihydrate. Calorimetry was used to experimentally determine the heat of solution for both reactions.
Procedure: This lab was performed based on the procedure outlined in “Exp #7 Calorimetry.” No changes to the procedure were made.
Data and Observations: All data and observations were recorded in the lab notebook. Pages from the lab notebook are attached to the lab.
Results …show more content…
The molar enthalpy of dehydration is not able to be determined in a one-step calorimetry experiment because the dissociation of ions occurs when the solution dissolves in water. Hess’s Law allows for the two thermochemical equations to be added resulting in a net equation, one that describes the molar enthalpy of dehydration. Calorimetry is using a tool, the calorimeter, which insulates the system from the environment. This allows for the changes of temperature to be observed with minimal heat loss to the environment. Calorimetry allows for the heat of the solution to be calculated since the heat capacity of the calorimeter is known and the change in temperature is observed. The heat capacity is the ability for the container to retain the heat the is produced or absorbed without allowing for the outside environment to impact the reaction. This closed system allows for easy calculations where q_rxn+q_water+q_calorimeter=0. This is important to the lab that the total heat lost and gained must all equal zero. It would be hard to calculate how much heat was lost in the world by the experiment, so isolating the system to the calorimeter allows for the …show more content…
This was confirmed by the values obtained from the Handbook of Chemistry and Physics. The experiment involved the use of calorimetry and Hess’s Law to calculate the molar enthalpy of dehydration. An important improvement to increase the accuracy of the data would be to use a digital thermometer with shorter intervals in recording the data, especially when the reaction is occurring. This would improve identifying the true final temperature of the system. Another improvement would be to use a calorimeter that better retains heat. This would also increase the accuracy of the final temperature that the solution obtains as less heat is lost to the