Calorimetry Lab Report Essay Example
06.03 Calorimetry: Lab Report
Before You Begin: You may either copy and paste this document into a word processing program of your choice or print this page.
Part I
The Dissolving of Solid Sodium Hydroxide in Water
Procedure:
1. Measure out approximately 200 mL of distilled water and pour it into the calorimeter. Stir carefully with a thermometer until a constant temperature is reached. Record the volume of water and the constant initial temperature of the water on your data table. 2. Place a plastic measuring trough on top of the digital balance, and then zero the balance (press the tare button) so that the mass of the trough will be "ignored" and will not be added to the total mass measured by the balance. 3. Measure out approximately three to five scoops of solid sodium hydroxide and record the mass to your data table. 4. Place the solid sodium hydroxide into the water in the calorimeter and replace the lid immediately. Stir gently until the solid is completely dissolved and record the highest temperature reached.
Data and Observations: 5. Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations that you made over the course of Part I. Volume of H2O | 200.0 mL H2O | Mass of NaOH | 2.535 g NaOH | Initial temperature in calorimeter | 24.2 °C | Final temperature in calorimeter | 27.8 °C |
Calculations:
Show your work and write a short explanation with each calculation. 1. Write out a balanced "equation" for the process you investigated in Part I, including phase symbols.
NaOH(s) + H2O(l) --> NaOH(aq) 2. Calculate the number of moles of sodium hydroxide dissolved. Show your work.
Moles NaOH = 2.535 grams NaOH X (1 mol/40.00 grams) = 0.06338 moles NaOH 3. Calculate the amount of energy involved in this dissolving process. Show your work. q = m c (T2-T1)
200 mL H2O X 1 g/1 mL = 200 g H2O c = 4.184 J/gC
T2 = 27.8 C
T1 =
Before You Begin: You may either copy and paste this document into a word processing program of your choice or print this page.
Part I
The Dissolving of Solid Sodium Hydroxide in Water
Procedure:
1. Measure out approximately 200 mL of distilled water and pour it into the calorimeter. Stir carefully with a thermometer until a constant temperature is reached. Record the volume of water and the constant initial temperature of the water on your data table. 2. Place a plastic measuring trough on top of the digital balance, and then zero the balance (press the tare button) so that the mass of the trough will be "ignored" and will not be added to the total mass measured by the balance. 3. Measure out approximately three to five scoops of solid sodium hydroxide and record the mass to your data table. 4. Place the solid sodium hydroxide into the water in the calorimeter and replace the lid immediately. Stir gently until the solid is completely dissolved and record the highest temperature reached.
Data and Observations: 5. Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations that you made over the course of Part I. Volume of H2O | 200.0 mL H2O | Mass of NaOH | 2.535 g NaOH | Initial temperature in calorimeter | 24.2 °C | Final temperature in calorimeter | 27.8 °C |
Calculations:
Show your work and write a short explanation with each calculation. 1. Write out a balanced "equation" for the process you investigated in Part I, including phase symbols.
NaOH(s) + H2O(l) --> NaOH(aq) 2. Calculate the number of moles of sodium hydroxide dissolved. Show your work.
Moles NaOH = 2.535 grams NaOH X (1 mol/40.00 grams) = 0.06338 moles NaOH 3. Calculate the amount of energy involved in this dissolving process. Show your work. q = m c (T2-T1)
200 mL H2O X 1 g/1 mL = 200 g H2O c = 4.184 J/gC
T2 = 27.8 C
T1 =