CHM1011 - Chemistry I - S1 2025
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| water | ||
| CuCl | → | Cu2+(aq) + 2Cl2-(aq) |
A student ended the experiment with 0.1452g of copper, having started with 0.2343g of CuCl2.2H2O.
Calculate the moles of pure copper (Cu) produced:
A student ended the experiment with 0.1452g of copper, having started with 0.2343g of CuCl2.2H2O.
Calculate the %yield of copper produced, i.e. the percentage recovery of copper compared to the expected amount.
(Hint: The reagents used are always in excess to the copper species (sodium hydroxide, sulfuric acid, and zinc). Hence, the copper species is always the limiting reagent. This means that the nCu=nCuCl2.2H2O at 100% yield.)
(Hint 2: If the copper produced was not adequately dried before weighing, then we may end up calculating a yield of >100%! Why is this?)
Calculations
Based on the experimental data provided, complete the following calculations.
A student ended the experiment with 0.1452g of copper, having started with 0.2343g of CuCl2.2H2O.
Calculate the moles of CuCl2.2H2O used:
Results
Experimental Data
Mass CuCl2.2H2O (g) | g |
|---|---|
Mass of Cu in CuCl2.2H2O (g) | g |
Mass of Copper recovered (g) | g |
% yield of Copper | % |
Observations
Type up a summary of your observations for each section.
- Section 2.1 (i) - Dissolution of Copper(II) chloride dihydrate:
- Section 2.1 (ii) - Copper(II) chloride to copper(II) hydroxide:
- Section 2.2 - Copper(II) hydroxide to copper(II) oxide:
- Section 2.3 - Copper(II) oxide to copper(II) sulfate:
- Section 2.4 - Copper(II) sulfate solution to copper:
When writing an aim, it should be in the format of the Goal (what do you want to achieve) and the Means (how you plan to achieve it).
Read over the exercise in your lab manual to assist you with completing the aim for this experiment. Record the aim in your laboratory notebook, so that you will be able to address it when you write the conclusion for your lab report.
Aim:
To investigate and observe different chemical transformations of
In the early morning when the temperature was 13.7 oC, a motorist measured her tyre pressure at 183 kPa. By noon the temperature in the tyres had reached 32.7 oC. What was the pressure (in kPa) in the tyres at noon assuming there was no change in volume?
Give your answer to three significant figures.
A micro-syringe used in gas chromatography has a maximum volume of 50 mL. A chemical reaction known to generate methane gas is sampled using the syringe twice. The first sample with a volume of 10.0 mL was determined to contain 7.52x10-7 moles of methane gas. If a second sample of 25.0 mL was taken, with the reaction at the same temperature and pressure, how many moles of gas are in the 25.0 mL sample?
Enter your answer to 3 significant figures using scientific notation - for example, 1.23E-4 represents 1.23x10-4. Do not enter units.
If a balloon has a volume of 1.333 L at a temperature of 11.7 C°, what will be the volume (L) of the balloon if the temperature is increased to 40.3 C°?
Give your answer to four significant figures.
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