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Report (any type)/Brief report
22/09/2021
change can be determined by using the equation: enthalpy change = mcΔT, where m is the mass of your solution, c is the , and ΔT is the change is temperature.
Thus, in order to determine or calculate the enthalpy change you will need to know all of these measurements or to find them all experimentally. Here’s a great video of an experiment conducted to calculate the enthalpy change!
Ehthalpy change for an aqueous solution can be determined experimentally. Utilizing a thermometer to measure the temperature change of the solution , (along with the mass of the solute) to determine the enthalpy change for an aqueous solution, as long as the reaction is carried out in a calorimeter or similar apparatus . You can use a coffee cup calorimeter.
Step 1. Measure the mass of in grams using a balance. I am dissolving solute Sodium Hydroxide. The mass I have taken is 4 g or 0.1 moles.
Step 2. Measure the volume of water. I am going to use 100 ml of water. Record the of water. Using Density and volume of water I can calculate the mass of water using formula;
Mass = Volume x Density ( let us assume the density of water to be 1g / ml, the mass of 100 ml of water is 100g.
Step 3. Pour the 100 ml of water in a coffee cup calorimeter, record the temperature of water , the initial temperature of water is ##27^o## C.
Step 4. Add 4 g of Sodium Hydroxide to the water. Dissolve the sodium Hydroxide using a stirrer and also record the temperature of solution. Let us assume that the final temperature of the solution is ##48^o## C
Step 5. In this dissolution experiment Sodium hydroxide dissolves in water and gives off heat energy to the surrounding water , which causes the temperature of water to go up from ##27^o## C to ##48^o## C. The change in temperature is ##48^o## C – ##27^o## C = ##21^o## C
Step 6. Use the formula Q = mass of water . specific heat of water . change in Temperature to calculate amount of heat gained by water.
Step 7 Q = 100 g . 4.18 J / ##g^oC##. ##21^o## C
Q = 8778 J or 8.778 kJ
Water has gained 8.778 kJ of heat energy from the salt, or salt has lost 8.778 kJ of heat energy to water. So energy lost by salt is -8.778 kJ.
Change in enthalpy = Q lost by salt / of moles of salt
= -8.778 kJ / 0.1 mol = -87.88 kj /mol
Check here for more information about different types of enthalpies
Here is a video on Calorimetry and how to determine ##DeltaH##.
I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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