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The following mechanism has been proposed for the gas phase reaction of nitrogen monoxide with bromine. step 1 fast: NO + Brz NOBr2 step 2 slow: NOBr2 + NO 2 NOBY (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"", where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
One possible mechanism for the gas phase reaction of hydrogen with nitrogen monoxide is: step 1 slow: H2(g) + 2 NO(g) + N20(9) + H20(9) step 2 fast: N20(9) + H2(g) → N2(9) + H20(9) (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]”"..., where '1' is understood (so don't write it) for m, n etc.) Rate =
The gas phase decomposition of dinitrogen pentoxide at 335 K N2Os(9) → 2 NO2(g) + 12 02(9) is first order in N2O5 with a rate constant of 4.70x10-3 s. If the initial concentration of N2O5 is 0.201 M, the concentration of N2O5 will be M after 360 s have passed.