The breakdown of a certain pollutant X in sunlight is known to follow first-order kinetics. An atmospheric scientist studying the process fills a 40.0 L reaction flask with a sample of urban air and finds that the partial pressure of X in the flask decreases from 0.66 atm to 0.14 atm over 13. hours. Calculate the initial rate of decomposition of X, that is, the rate at which X was disappearing at the start of the experiment. Round your answer to 2 significant digits. 0 atm S 0 x10 X

Decomposition of NH3 in presence of molybdenum is a zero-order reaction with a rate constant of 2.36x10-2 mol L-1 s-1 at a certain temperature. An experiment was run at this temperature where [NH3]0 = 3.40 mol L-1. What is rate after 25 s?

rate constant 1 H₂(g) + 2NO(g) N₂O(g) + H₂O(g) k₁ 2 H₂(g) + N₂O(g) → N₂(g) + H₂O(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, K₂, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. step elementary reaction t k = A 00 X

For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C 2 H,O2(aq)– →2 H,O(1) + O2(g) the average rate of disappearance of H,O, over the time period from t = 0 min to t= 635 min is found to be 5.54×10-5 M min1. The average rate of formation of O, over the same time period is M min.