Question

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Answer 1

Using the stoichiometry of the balanced equation, 2.6 moles of water are produced when 1.7 moles of
`NH_3` are consumed.

In stoichiometry, the balanced chemical equation provides the molar ratios between reactants and products in a chemical reaction. For the given balanced equation \(2 \text{NH}_3 \rightarrow 3 \text{H}_2\text{O}\), it indicates that 2 moles of ammonia (NH₃) produce 3 moles of water (H₂O).

To find out how many moles of water are formed when 1.7 moles of NH₃ are consumed, set up a proportion using the molar ratios from the balanced equation. The ratio
`\( \frac{3 \text{ moles H}_2\text{O}}{2 \text{ moles NH}_3} \)` represents the stoichiometric relationship.

Multiply this ratio by the given amount of NH₃ (1.7 moles):

`\[ 1.7 \text{ moles NH}_3 * \frac{3 \text{ moles H}_2\text{O}}{2 \text{ moles NH}_3} = 2.55 \text{ moles H}_2\text{O} \]`

Rounding to the nearest tenth, the result is 2.6 moles of water (H₂O) produced when 1.7 moles of NH₃ are consumed in the reaction. This calculation ensures a quantitative understanding of the reactants' conversion to products based on the principles of stoichiometry.