Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: H2 (g) + 2NO (g) ? N2O (g) + H2O (g) [NO] (M) | 0.30 | 0.60 | 0.60 [H2] (M) | 0.35 | 0.35 | 0.70 Rate (mol L^-1 s^-1) | 2.835 !! 10^-3 | 1.134 !! 10^-2 | 2.268 !! 10^-2 Determine the following information using the data in the table above and fill in the answer (1-4 below): 1. Rate = (Use ^ before a number for exponents) (4 pts) 2. Rate constant (type A, B, or C in blank) = (2 pts) A. 2.7 x 10^-2 L^2 mol^-2 s^-1 B. 9.0 x 10^-2 L^2 mol^-2 s^-1 C. 12.2 x 10^-2 L^2 mol^-2 s^-1 3. H2 reaction order = (2 pts) 4. NO reaction order = (2 pts)
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We need to find the rate law expression. We can use the given data to find the relationship between the concentrations and the rate. Let's call the rate constant k, the order of the reaction with respect to H2 as x, and the order of the reaction with respect to NO Show more…
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Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: $\mathrm{H}_{2}(g)+2 \mathrm{NO}(g) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{H}_{2} \mathrm{O}(g)$ Determine the rate law, the rate constant, and the orders with respect to each reactant from the following data:
Nitrogen monoxide reacts with hydrogen gas to produce nitrogen and water vapor. The mechanism is believed to be: Step 1: 2NO(g) → N2O2(g) (slow) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) Step 3: N2O(g) + H2(g) → N2(g) + H2O(g) Write an overall balanced equation for this process (show your work). Identify the reaction intermediates. Write the rate equation for this reaction.
Alkendra S.
Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, $\mathrm{N}_{2} \mathrm{O},$ and water. $$ 2 \mathrm{NO}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{H}_{2} \mathrm{O}(g) $$ In a series of experiments, the following initial rates of disappearance of NO were obtained: Find the rate law and the value of the rate constant for the reaction of NO.
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