Example of a laboratory chemistry experiment report.

Title: Determination of the Molar Mass of a Gas

Objective:
The objective of this experiment is to determine the molar mass of an unknown gas by measuring its density and using the ideal gas law equation.

Materials:
- Gas sample
- Gas syringe
- Balance
- Thermometer
- Barometer
- Graduated cylinder
- Water bath
- Stopwatch

Procedure:
1. Weigh the gas syringe and record its mass.
2. Fill the gas syringe with the gas sample and record the volume.
3. Measure the temperature of the gas sample using the thermometer.
4. Measure the atmospheric pressure using the barometer.
5. Fill the graduated cylinder with water and invert it in the water bath.
6. Displace the water in the graduated cylinder with the gas sample and record the volume of water displaced.
7. Calculate the density of the gas sample using the formula: density = mass/volume.
8. Use the ideal gas law equation (PV = nRT) to calculate the molar mass of the gas sample.

Results:
- Mass of gas syringe: 10.5 g
- Volume of gas sample: 50 mL
- Temperature of gas sample: 25°C
- Atmospheric pressure: 1 atm
- Volume of water displaced: 20 mL
- Density of gas sample: 0.21 g/mL
- Molar mass of gas sample: 44.8 g/mol

Conclusion:
The molar mass of the unknown gas sample was determined to be 44.8 g/mol. This value is close to the expected molar mass of oxygen gas (O2), which is 32 g/mol. The slight discrepancy may be due to experimental errors or impurities in the gas sample. Overall, the experiment was successful in determining the molar mass of the gas sample using the ideal gas law equation.

Laboratory Chemistry Experiment Report

Experiment Title: Synthesis and Characterization of Copper(II) Sulfate Pentahydrate

Name: Jane Doe

Instructor: Dr. John Smith

Date: March 10, 2023

Objective:

The objective of this experiment was to synthesize copper(II) sulfate pentahydrate from copper(II) oxide and sulfuric acid, and to characterize the product using various analytical techniques.

Materials:

- Copper(II) oxide (CuO)
- Sulfuric acid (H2SO4)
- Distilled water
- Beaker
- Evaporating dish
- Hot plate
- Magnetic stirrer
- Volumetric flask
- UV-Vis spectrophotometer
- X-ray diffractometer

Procedure:

1. Weigh out 0.500 g of CuO into a beaker.
2. Add 10 mL of concentrated H2SO4 to the beaker and stir until a paste forms.
3. Add 50 mL of distilled water to the beaker and heat the solution on a hot plate while stirring.
4. Continue heating and stirring until the solution turns a deep blue color and all of the CuO has dissolved.
5. Filter the solution through a filter paper to remove any impurities.
6. Evaporate the filtrate to dryness in an evaporating dish.
7. Dissolve the crystals in 100 mL of distilled water in a volumetric flask.

Analysis:

- UV-Vis Spectroscopy: The UV-Vis spectrum of the copper(II) sulfate solution showed an absorption peak at 600 nm, which is characteristic of the d-d transition of the Cu(II) ion.
- X-ray Diffraction: The X-ray diffraction pattern of the copper(II) sulfate crystals showed sharp peaks indicating the formation of a crystalline solid. The pattern matched the reference pattern for copper(II) sulfate pentahydrate.

Results:

The yield of copper(II) sulfate pentahydrate was 0.750 g (92.5% yield). The crystals were blue and had a density of 1.90 g/cm3.

Conclusion:

The experiment was successful in synthesizing copper(II) sulfate pentahydrate from copper(II) oxide and sulfuric acid. The product was characterized using UV-Vis spectroscopy and X-ray diffraction, and the results confirmed the formation of the desired compound.