Metallic copper is formed when aluminum reacts with copper (II) sulfate. What is the theoretical...
Question:
Metallic copper is formed when aluminum reacts with copper (II) sulfate. What is the theoretical yield of copper if 54.0 g of Al react with excess {eq}CuSO_4 {/eq}?
Given the equation for reaction is
{eq}2Al + 3CuSO_4 \to Al_2(SO_4)_3+ 3Cu {/eq}.
Using Stoichiometric Ratios:
It is possible to determine the amount of product that is possible to form given the amount of reactant. This is because the reactants react in a specific ratio to produce a specific amount of products. The ratios which are used for these calculations can be found in the balanced reaction equation. The ratio of the coefficients in front of the two chemicals in question will be the ratio of the number of moles of the two chemicals. The ratio in the number of moles matches the ratios of the coefficients because the number of moles is just a way to count the number of atoms/molecules in a sample and so any ratio that is true for the number of atoms/molecules must also be true for the number of moles.
Answer and Explanation:
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View this answerThe molar mass of Al is 26.981538 g/mol. The number of moles of Al is
{eq}n = \frac {54.0 \ g}{26.981538 \ g/mol} \\ n = 2.00 \ mol {/eq}
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