Cu (s) +2Ag(NO 3 ) (aq) →2Ag (s) +Cu(NO 3 ) 2 (aq) C, u, start subscript, left parenthesis, s, right parenthesis, end subscript, plus, 2, A, g, left parenthesis, N, O, start subscript, 3, end subscript, right parenthesis, start subscript, left parenthesis, a, q, right parenthesis, end subscript, right arrow, 2, A, g, start subscript, left parenthesis, s, right parenthesis, end subscript, plus, C, u, left parenthesis, N, O, start subscript, 3, end subscript, right parenthesis, start subscript, 2, end subscript, start subscript, left parenthesis, a, q, right parenthesis, end subscript8.9 moles of Cu react with 15.6 moles of AgNO3. What is the excess reactant and how much of it remains?
Question
Cu (s) +2Ag(NO 3 ) (aq) →2Ag (s) +Cu(NO 3 ) 2 (aq) C, u, start subscript, left parenthesis, s, right parenthesis, end subscript, plus, 2, A, g, left parenthesis, N, O, start subscript, 3, end subscript, right parenthesis, start subscript, left parenthesis, a, q, right parenthesis, end subscript, right arrow, 2, A, g, start subscript, left parenthesis, s, right parenthesis, end subscript, plus, C, u, left parenthesis, N, O, start subscript, 3, end subscript, right parenthesis, start subscript, 2, end subscript, start subscript, left parenthesis, a, q, right parenthesis, end subscript8.9 moles of Cu react with 15.6 moles of AgNO3. What is the excess reactant and how much of it remains?
Solution
To solve this problem, we need to first understand the stoichiometry of the reaction. According to the balanced chemical equation, one mole of Cu reacts with two moles of AgNO3 to produce two moles of Ag and one mole of Cu(NO3)2.
Given that we have 8.9 moles of Cu and 15.6 moles of AgNO3, we can see that not all of the Cu will react. This is because, according to the stoichiometry of the reaction, we would need 17.8 moles of AgNO3 to fully react with the 8.9 moles of Cu.
Therefore, Cu is the limiting reactant because it will be completely consumed before all of the AgNO3 has had a chance to react.
To find out how much AgNO3 remains, we need to calculate how much AgNO3 reacts with the 8.9 moles of Cu. According to the stoichiometry of the reaction, one mole of Cu reacts with two moles of AgNO3. Therefore, 8.9 moles of Cu will react with 17.8 moles of AgNO3.
Given that we started with 15.6 moles of AgNO3, and 17.8 moles of it would have reacted, we actually have an excess of AgNO3. Therefore, there is no AgNO3 remaining, and all of the Cu and AgNO3 react completely.
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