How do you find heat of solvation of NH4Cl?
Answers
Enthalpy 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.
Measure the mass of solute in grams using a balance. I am dissolving solute Ammonium chloride The mass I have taken is 5.4 g or 0.1 moles.
Measure the volume of water. I am going to use 100 ml of water. Record the Density 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).
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.
Add 5.4 g of Ammonium chloride to the water. Dissolve the Ammonium chloride using a stirrer and also record the temperature of solution. Let us assume that the final temperature of the solution is
19
o
C
In this dissolution experiment Ammonium chloride dissolves in water and absorbs heat energy from the surrounding water , which causes the temperature of water to go down from
27
o
C to
19
o
C. The change in temperature is
19
o
C -
27
o
C = -
8
o
C
Use the formula Q = mass of water . specific heat of water . change in Temperature to calculate amount of heat gained by water.
Q = 100 g . 4.18 J /
g
o
C
. -
8
o
C
Q = -3344 J or -3.34 kJ
Water has lost -3.34 kJ of heat energy to the salt, or salt has gained + 3.34kJ of heat energy from water. So energy gained by salt is + 3.34 kJ.
Change in enthalpy = Q gained by salt / # of moles of salt
= +3.34 kJ / 0.1 mol = +33.4 kj /mol
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Enthalpy 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.
Measure the mass of solute in grams using a balance. I am dissolving solute Ammonium chloride The mass I have taken is 5.4 g or 0.1 moles.
Measure the volume of water. I am going to use 100 ml of water. Record the Density 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).
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.
Add 5.4 g of Ammonium chloride to the water. Dissolve the Ammonium chloride using a stirrer and also record the temperature of solution. Let us assume that the final temperature of the solution is
19
o
C
In this dissolution experiment Ammonium chloride dissolves in water and absorbs heat energy from the surrounding water , which causes the temperature of water to go down from
27
o
C to
19
o
C. The change in temperature is
19
o
C -
27
o
C = -
8
o
C
6.Use the formula Q = mass of water . specific heat of water . change in Temperature to calculate amount of heat gained by water.
7.Q = 100 g . 4.18 J /
g
o
C
. -
8
o
C
Q = -3344 J or -3.34 kJ
Water has lost -3.34 kJ of heat energy to the salt, or salt has gained + 3.34kJ of heat energy from water. So energy gained by salt is + 3.34 kJ.
Change in enthalpy = Q gained by salt / # of moles of salt
= +3.34 kJ / 0.1 mol = +33.4 kj /mol