Consider the following hypothetical aqueous reaction: A(aq) → B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected. Calculate the average rate of appearance for B in units of M/s between 20 and 40 seconds. Time (sec) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031

What is the pH of a 0.050M solution of benzoic acid, C6H5COOH, which has a Ka = 6.3 x 10-5?

What is the pH of a 0.075M solution of ethylamine, C2H5NH2, which has a Kb = 6.4 x 10-4?

From the following values for a calculated rate constant, which one would be for a second-order reaction?

What is the pH of a solution prepared by taking 10.0 mL of 0.45 M HClO4 and diluting it to a final volume of 250 mL?

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

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

The hydrogen carbonate ion (HCO3-) is amphiprotic in water. If HCO3- is the Brønsted-Lowry base, what is the conjugate acid?

The rate of a particular reaction was measured at several different temperatures. A graph of ln k versus 1/T gives a slope of -2.82 x 103 K. Calculate the activation energy for the reaction given R is the gas constant (8.314 J/mol-K) given Ea = -slope x R.

Based on their activation energies and energy changes and assuming that all collision factors are the same, rank to the following reactions from slowest to fastest. (i) Ea= 45 kJ/mol; ΔE=–25 kJ/mol (ii) Ea= 35 kJ/mol; ΔE=–10 kJ/mol (iii) Ea= 55 kJ/mol; ΔE=10 kJ/mol