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A reaction involves 2 different reactants and both reactants are first order. How does the rate change if the concentration of one reactant is doubled while the concentration of the second reactant is held constant?

The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5 → 4 NO2 + O2. The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 × 10–3 s–1. What is the rate of reaction when [N2O5] = 1.00 M?

Calculate the concentration of OH-(aq) in a solution in which [H+] is 0.010 M.

What is the acid dissociation constant, Ka, for propionic acid, C2H5COOH in water?

With the polyprotic acid like H3PO4, the dissociation of which hydrogen atom gives the largest Ka value?

Calculate the concentration of H+(aq) in a solution in which [OH-] is 0.010 M.

A solution contains three anions with the following concentrations: 0.20 M CrO42–, 0.10 M CO32–, and 0.010 M Cl–. If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 (Ksp = 1.2 × 10–12), Ag2CO3 (Ksp = 8.1 × 10–12), or AgCl (Ksp = 1.8 × 10–10)?

For a saturated solution of Co(OH)2, what happens when a strong acid is added?

The first-order decomposition of N2O5 was studied at a particular temperature and found to have a rate constant of 6.2 x 10-4s-1. What is the half-life for the decomposition under these conditions?

Identify the Brønsted-Lowry base in the following reaction, (CH3)3N(aq) + H2O(l) → (CH3)3NH+(aq) + OH-(aq).