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Write a balanced reaction for which the following rate relationships are TRUE.             Rate =  =  = –  

The rate constant for the first-order decomposition of N2O is 3.40 s-1. What is the half-life of the decomposition?

Reaction rate can change with _______ I.     temperature. II.   the addition of a catalyst. III.  reactant concentrations.

Place the following in order of increasing entropy at 298 K.

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system?                                   CuS(s) + O2(g) ⇌ Cu(s) + SO2(g)

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1. If the initial concentration of cyclopropane is 1.33 M, what is the concentration of cyclopropane after 644 s?

A reaction is followed and found to have a rate constant of 3.36 × 104 M-1s-1 at 344 K and a rate constant of 7.69 M-1s-1 at 219 K. Determine the activation energy for this reaction.

A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? 1st step: A + B → 2C + D      slow 2nd step: C → E            fast 3rd step: D → 2F           fast

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(g) + H2O(g) ⇌ C2H5OH(g)   Kc = 9.0 × 103 [C2H4]eq = 0.015 M                        [C2H5OH]eq = 1.69 M

Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g)    ΔH = -1,036 kJ ΔS = -153.2 J/K