Dinitrogen Pentoxide, N2O5, decomposes when heated to give in carbon tetrachloride solvent.   N2O5(g) →  2 NO2(g) + 1/2 O2(g) The reaction is first order. If the rate constant for the decomposition is 8.4x10-4/min what is the half-life, in hr, for the decomposition? Express your answer to one decimal place.

Aa.104.

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

Chlorine dioxide, CIO₂, is a reddish-yellow gas that is soluble in water. In basic solution it gives CIO3 and ClO₂ ions. 2 CIO₂(aq) + 2 OH(aq) → CIO3(aq) + ClO₂ (aq) + H₂O(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO₂ was determined. Use the data here to determine the order of the reaction for CIO₂ and OH, and the value of the rate constant. [CIO2]init [OH Jinit Initial Rate, mol/(Los) Exp. 1 0.030 Exp. 2 0.060 Exp. 3 0.030 Order for CIO₂: Order for OH": Rate constant = 0.030 0.030 0.060 0.0062 0.0248 0.0124