Question

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Answer 1

To find out how many moles of NO can be made when 6.5 moles of
`HNO_3` are consumed, we use the mole ratio between
`HNO_3` and NO.

In the given reaction
`\(3 \text{Cu} + 8 \text{HNO}_3 \rightarrow 3 \text{Cu(NO}_3\text{)}_2 + 2 \text{NO} + 4 \text{H}_2\text{O}\)`, the mole ratio between
`HNO_3` and NO is 8:2. This ratio implies that for every 8 moles of
`HNO_3` consumed, 2 moles of NO are produced.

If 6.5 moles of
`HNO_3` are consumed, we can use the mole ratio to determine the moles of NO produced:

`\[\text{Moles of NO} = (6.5 \, \text{moles HNO3}) * \left( \frac{2 \, \text{moles NO}}{8 \, \text{moles HNO3}} \right) = 1.625 \, \text{moles NO}\]`

Rounding to the nearest tenth, approximately 1.6 moles of NO are produced.

This calculation showcases the stoichiometric relationship between reactants and products in a chemical reaction. The coefficients in the balanced equation establish the mole ratios, allowing for the conversion of moles of one substance to moles of another. In this case, it helps determine the amount of NO produced when a specific quantity of
`HNO_3` is consumed. Such stoichiometric calculations are fundamental in understanding and predicting chemical reactions in a quantitative manner.