Good Report On Heat Of Solution Of Cacl2

Introduction

There are often changes during chemical reactions involving solids and aqueous solutions. These changes are due to the reaction between the different properties of the liquid and the solid materials, which result in an increase or reduction in temperatures.
These reactions are usually observed using specialized laboratory equipments, which normally maintain certain environmental conditions. This gives a report concerning an experiment that used a calorimeter to measure the amount of heat which was released or absorbed during a chemical process (Harmathy, 1985). This will be measured using a calorimeter, which will record the rise or drop in temperature as will be captured using an inbuilt thermometer in the calorimeter.

Hypothesis

The reaction will lead to the formation of new chemical bonds hence energy would be given out leading to a rise in temperature of the solution when CaCl2 is dissolved in water.

There will be an increase in mass of the liquid after the chemical reaction.

What is a calorimeter
This refers to an instrument that measures the amount of heat which is transferred or emitted by an object during a chemical reaction.
It is also a device that is used to measure the thermal effects that occur during biological, physical or chemical processes.

What are the principles of calorimetry that make it a good way to measure energy changes?

Calorimeters can accommodate chemical reactions involving solids and liquids at room temperatures. This is because it has properties that can accommodate both endothermic and exothermic reactions.
Calorimeters work at constant temperatures, hence allows the device to measure the reaction within its heat sink. The calorimeters also have very high degree of sensitivity that enables it to measure the conduction of heat as it travels during the chemical reaction processes (Cazes & Ewing, 2005).

Calorimetry occurs well in three modes of operation.

Isothermal operation where the temperatures within the environment are maintained at constant temperatures
Isoperibol operation: This case permits the samples to change in a given constant temperature within the environment.
Adiabatic operation: This principle occurs where there is no heat exchange between the environment and the sample during a chemical change.
On the other hand, their in-built functions to help in determining the difference between the heat exchanged between the surrounding environment and the sample itself (Mehling & Cabeza, 2008).

Other principles:

Construction principle:
A single measuring system that is calibrated to eliminate systematic errors associated with thermodynamics. The design is also made in a way that it reduces external and internal noise influences as well as transient fluctuations that may cause unsuspected behavior during the reaction process.
Calorimeters are constructed in a way that they have internal thermometers that measure the changes in temperatures of the solution. The amount of heat released will lead to a rise in temperature levels and will be captured by the in-built thermometer.
On the other hand, a calorimeter can also be used to measure the enthalpy change that occurs during the reaction between the calcium chloride and water.
Calorimeters are used to measure both exothermic and endothermic reactions. They have a wider use in calorimetry, with their application widely used in modern chemistry.

How will a calorimeter be useful to measure the heat (enthalpy) of solution of CaCl2?

Calorimeters are designed in a way that they allow temperatures to rise, in instances of exothermic reactions while also allows temperatures to fall during endothermic reactions.

What is expected to happen to the temperature of the solution as CaCl2 is dissolved in water?

The temperature of the solution in expected to rise when calcium chloride is dissolved in water, in a calorimeter (Ebbing & Gammon, 2005). There will also be an enthalpy change when the reaction occurs in water.

References

Cazes, J., & Ewing, G. W. (2005). Ewing's analytical instrumentation handbook. New York: Marcel Dekker.
Ebbing, D. D., & Gammon, S. D. (2008). General chemistry. Boston: Houghton Mifflin.
Mehling, H., & Cabeza, L. F. (2008). Heat and cold storage with PCM: An up to date introduction into basics and applications. Berlin: Springer.
Symposium on Application of Fire Science to Fire Engineering., & Harmathy, T. Z. (2011). Fire safety, science and engineering. Philadelphia, Pa: American Society for Testing and Materials.