The intent of the experiment is to cipher the heat content alteration happening in the first of reaction of Na hydrated oxide with hydrochloric acid and Na hydrated oxide with ammonium chloride. Using Hess’ Law and the consequences for the enthalpy alteration of the first two reactions should give the enthalpy alteration of the 3rd reaction of ammonium hydroxide with hydrochloric acid.
Procedure:
Part 1:
Concept a calorimeter of two nested stereo system cups where the screen has a hole to fir a thermometer. Measure 50ml distilled H2O at room temperature into the calorimeter. Measure the temperature. Heat 75ml of distilled H2O to 70 grades Celsius and pour it into the calorimeter. Record the temperature alteration every 20 seconds for 3 proceedingss. Part2:
Find the mean initial temperature of Na hydrated oxide and hydrochloric acid. Determine the temperature alteration occurs when you mix 50ml of 2M of each solution utilizing a magnetic stirring motor. Record the temperature every 20 seconds for 3 proceedingss. Repeat this procedure for the other two reactions.
Graph of Temperature Change in Water
Graph of Temperature Changes in Chemical reactions:
1. Sodium Hydroxide with Hydrochloric Acid
2. Sodium Hydroxide with Ammonium Chloride
3. Hydrochloric Acid with Ammonia
Average Temperature of Water:
Trial 1 Average: 45. 41 grades Celsius
Trial 2 Average: 44. 58 grades Celsius
Average of Tests: 44. 995 grades Celsius
Heat Absorbed by Calorimeter: -525. 87 Joules
Specific Heat of the Calorimeter: 27. 68J/C
Enthalpy Change:
Chemical reaction 1: . 0587570 kJ/g
Chemical reaction 2: . 059825 kJ/g
Chemical reaction 3: . 05366 kJ/g
Net Ionic Chemical reactions:
1. OH + H ( H2O
2. OH + NH4 ( H2O + NH3
3. H + NH3 ( NH4
Hess’ Law
2. OH +NH4 ( H2O + NH3
~ 1. OH + H ( H2O
( NH4 – H ( NH3 ) = ( NH3 + H ( NH4 ) = Reaction 3
0. 059825 kJ/g – 0. 058757kJ/g =
