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Sia

青州's Question
Chemistry
Posted 2 months ago

The reaction of nitric oxide with hydrogen at 1280C1280^{\circ} \mathrm{C} is
2NO(g)+2H2(g)N2(g)+2H2O(g)
2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)


From the following data collected at this temperature, determine (a) the rate law, (b) the rate constant, and (c) the rate of the reaction when [NO]=12.0×103M[\mathrm{NO}]=12.0 \times 10^{-3} \mathrm{M} and
[H2]=6.0×103M
\left[\mathrm{H}_{2}\right]=6.0 \times 10^{-3} \mathrm{M} \text {. }

\begin{tabular}{cccc} 
Experiment & {[NO](M)[\mathbf{N O}](M)} & {[H2](M)\left[\mathbf{H}_{2}\right](M)} & Initial Rate (M/s)(M / \mathbf{s}) \\
\hline 1 & 5.0×1035.0 \times 10^{-3} & 2.0×1032.0 \times 10^{-3} & 1.3×1051.3 \times 10^{-5} \\
2 & 10.0×10310.0 \times 10^{-3} & 2.0×1032.0 \times 10^{-3} & 5.0×1055.0 \times 10^{-5} \\
3 & 10.0×10310.0 \times 10^{-3} & 4.0×1034.0 \times 10^{-3} & 10.0×10510.0 \times 10^{-5}
\end{tabular}
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Answer from Sia
Posted 2 months ago
Solution
1
Determine the order with respect to NO: Compare experiments 1 and 2 where the concentration of H2\mathrm{H_2} is constant. Calculate the rate order with respect to NO\mathrm{NO} by using the initial rates and concentrations of NO\mathrm{NO}
2
Determine the order with respect to H₂: Compare experiments 2 and 3 where the concentration of NO\mathrm{NO} is constant. Calculate the rate order with respect to H2\mathrm{H_2} by using the initial rates and concentrations of H2\mathrm{H_2}
3
Write the rate law: Using the orders determined in steps 1 and 2, write the rate law expression
4
Calculate the rate constant (k): Use the given rate constant value to confirm the rate law
5
Calculate the rate of the reaction: Use the rate law and the given concentrations of NO\mathrm{NO} and H2\mathrm{H_2} to calculate the rate of the reaction
1 Answer
The rate law is Rate = k[NO]2[H2]k[\mathrm{NO}]^2[\mathrm{H_2}]
2 Answer
The rate constant (k) is 6.0×103M2s16.0 \times 10^3 \, \mathrm{M^{-2}s^{-1}}
3 Answer
The rate of the reaction is 4.32×104M/s4.32 \times 10^{-4} \, \mathrm{M/s}
Key Concept
The rate law for a reaction relates the rate of the reaction to the concentrations of the reactants and includes a rate constant (k) and reaction orders (m and n).
Explanation
The rate law is determined by comparing the initial rates and reactant concentrations from different experiments. The rate constant is a proportionality constant that relates the rate of a reaction to the concentrations of the reactants raised to their respective orders in the rate law.

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