**Question 10: Reaction Rate Calculation**Consider the chemical reaction:\[ 2\text{NH}_3(\text{g}) \rightarrow \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \]If the rate of change of the concentration of hydrogen gas (\(\Delta[\text{H}_2]/\Delta t\)) is \(0.030 \, \text{M} \cdot \text{s}^{-1}\), determine the rate of change of the concentration of ammonia (\(\Delta[\text{NH}_3]/\Delta t\)).To solve this, use the stoichiometric relationships from the balanced chemical equation. The relationship between the rates for each component can be derived from the coefficients:\[ \text{Rate of } \text{H}_2 = 3 \times \text{Rate of NH}_3 \]Thus, knowing the rate of formation of \(\text{H}_2\), the rate of disappearance of \(\text{NH}_3\) can be calculated as:\[ \Delta[\text{NH}_3]/\Delta t = \text{Rate of } \text{H}_2 / 3 \]\[ \Delta[\text{NH}_3]/\Delta t = 0.030 \, \text{M} \cdot \text{s}^{-1} / 3 \]\[ \Delta[\text{NH}_3]/\Delta t = 0.010 \, \text{M} \cdot \text{s}^{-1} \]Therefore, the rate of change of concentration of ammonia (\(\Delta[\text{NH}_3]/\Delta t\)) is \(0.010 \, \text{M} \cdot \text{s}^{-1}\).

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10). Consider this reaction: 2NH3(g) → N2(g) + 3H2(g) If the rate A[H2]/At is 0.030 M-1.s-1, then A[NH3]/At is

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