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CHM1011 - Chemistry I - S1 2025
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Upon the addition of sodium hydroxide solution to the copper(II) chloride solution, dark blue precipitate immediately started to form. After addition of all the sodium hydroxide, the entire system was an opaque dark blue suspension.
Upon addition of water to the green/blue copper(II) chloride (and slight shaking), a light blue transparent solution was formed.
| Heat | ||
| Cu(OH)2(s) | → | CuO(s) + H2O(g) |
2CuO(s) + 2H2SO4(aq) → 2CuSO5(aq) + 2H2(g)
| 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:
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:
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?)