Consider the following reaction: 2O3(g)-->3O2(g) The rate law for this reaction is as follows: Rate=k[O3]^2            ----            [O2] Suppose that a 1.0 L reaction vessel initially contains 1.0 mol ofO3 and 1.0 mol of O2. What fraction of the O3 will have reactedwhen the rate falls to one-half of its initial value?

The rate constant for the reaction is 0.200 M-! · s-! at 200 °C. A products If the initial concentration of A is 0.00780 M, what will be the concentration after 105 s? [A] = M * TOOLS x10

Consider the reaction below which can occur during the reforming process when manufacturing high octane gasoline:   3 C4H4  → 2 C6H6   or:  3 cylclobutadience → 2 benzene The average rate of appearance of benzene is given by Δ[benzene]/Δt.  If we compare the rate of appearance of benzene and the rate of disappearance of cyclobutadiene, we get  Δ[benzene]/Δt = ____________×(-Δ[cyclobutadiene]/Δt).  What should be written in the blank?     Question 1 options:   A)  -2/3   B)  +2/3   C)  -3/2   D)  +1   E)  +3/2

Nitrogen monoxide reacts with oxygen to give nitrogen dioxide. 2NO(9) + 02 (9) → 2NO: (9) The rate law is A[NO] At - k[NO]°[02] where the rate constant is 1.16 x 10-5 L/(mol? . s) at 339°C. A vessel contains NO and Oz at 339°C. The initial partial pressures of NO and Oz are 157 mmHg and 348 mmHg, respectively. What is the rate of decrease of partial pressure of NO? (Hint: From the ideal gas law, obtain an expression for the molar concentration of a particular gas in terms of its partial pressure.) Rate =