Given the following chemical equation:
3 Cu + 8 HNO3 = 3 Cu(NO3)2 + NO +
4 H2O.
How many moles of HNO3 are required to react with 6 moles of Cu?
Let's see now. According to the equation, 3 mols Cu use 8 mol HNO3, so 6 mols Cu will use ?? mols HNO3.
To determine how many moles of HNO3 are required to react with 6 moles of Cu, we need to use the stoichiometry of the balanced chemical equation.
In the balanced equation, the coefficients in front of the compounds represent the mole ratios between them. In this case, the coefficient of Cu is 3, and the coefficient of HNO3 is 8. This means that for every 3 moles of Cu, 8 moles of HNO3 are required for the reaction.
To find the moles of HNO3 needed when 6 moles of Cu are present, we can set up a proportion using the mole ratio:
(8 moles HNO3 / 3 moles Cu) = (x moles HNO3 / 6 moles Cu)
To solve for x (the unknown moles of HNO3), we can cross-multiply and then divide:
8 moles HNO3 * 6 moles Cu = 3 moles Cu * x moles HNO3
48 moles of HNO3 = 3x
Dividing both sides by 3:
48 moles HNO3 / 3 = x moles HNO3
16 moles HNO3 = x moles HNO3
Therefore, 16 moles of HNO3 are required to react with 6 moles of Cu.