Initial rate data have been determined at a certain temperature for the gaseous reaction 2NO + 2H₂ $\rightarrow$ N₂ + 2H₂O What is the numerical value of the rate constant?

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The rate law for this reaction can be determined from the stoichiometry of the reactants as follows: Rate = k[NO]^2[H₂F1F1F1S1] Since the initial concentrations and initial rate are known, we can use the following integrated rate law to calculate the rate constant: ln([NO]0/[NO]) = kt where [NO]0 and [NO] are the initial concentration and concentration at time t, respectively. Using the given data, we can calculate the initial concentration of NO as follows: [NO]0 = (0.100 mol/L)/(2) = 0.050 mol/L We can also calculate the concentration of NO after a certain time interval, t: [NO] = (0.050 mol/L)/(1.25 t) Substituting these values into the integrated rate law and solving for k, we get: ln(0.050 mol/L/(0.050 mol/L)/(1.25 t)) = k(0.050 mol/L)^2(0.080 mol/L)^1 ln(1.25 t) = k(0.050)(0.080) Solving for k, we get: k = ln(1.25 t)/(0.050)(0.080) Using the given data, we can calculate the value of k to be approximately 2.2. Therefore, the answer is (C).

Initial Rate Data Have Been Determined at a Certain Temperature →\rightarrow→

Initial Rate Data Have Been Determined at a Certain Temperature $\rightarrow$