A student is performing an experiment in the laboratory to determine the oxidation of copper (Cu). Cu reacts with oxygen in the air to formCuO in thefollowing reaction: Cu (s) + O2(g) →CuO (s) The student weighted 1.528gof Cu (s)powderin a crucible and heatedthe sample with a Bunsen burner.Even by using the Cuinpowderform and heating the sample there is unreacted Cu left in the crucible.After heating the student weighted the substance inside the crucible to be 3.647g. 1) If the student weighted 3.647 g of substance in the crucible. Calculate how much of this is unreacted Cu (s) and how much is CuO (s). (Hint: use the balanced chemical equation). 2) Once you know the amount of CuO (s) obtained in this experiment, calculate the percent yieldof CuO in this experiment.
A student is performing an experiment in the laboratory to determine the oxidation of copper (Cu). Cu reacts with oxygen in the air to formCuO in thefollowing reaction:
Cu (s) + O2(g) →CuO (s)
The student weighted 1.528gof Cu (s)powderin a crucible and heatedthe sample with a Bunsen burner.Even by using the Cuinpowderform and heating the sample there is unreacted Cu left in the crucible.After heating the student weighted the substance inside the crucible to be 3.647g.
1) If the student weighted 3.647 g of substance in the crucible. Calculate how much of this is unreacted Cu (s) and how much is CuO (s). (Hint: use the balanced chemical equation).
2) Once you know the amount of CuO (s) obtained in this experiment, calculate the percent yieldof CuO in this experiment.
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