Compare the average reaction rate measured over an initial, short time interval to one measured over a long time interval.

Explain what the reaction rate indicates about a particular chemical reaction.

Interpret how the speed of a chemical reaction is related to the spontaneity of the reaction.

Compare the concentrations of the reactants and products during the course of a chemical reaction (assuming no additional reactants are added).

Relate collision theory to reaction rate.

Explain what the reaction rate indicates about a particular chemical reaction.

Explain what the rate law for a chemical reaction tells you about the reaction.

Design an experiment based on solubilities to demonstrate which of two ions, $\mathrm{Mg}^{2+}$ or $\mathrm{Pb}^{2+}$, is contained in an aqueous solution.

Solubility information about ionic compounds is given in Tables $\mathbf{R - 3}$ and $\mathbf{R}-8$ in the Student Resources appendix.

A sample of ammonia $\left(\Delta H_{\text {solid }}=-5.66 \mathrm{kJ} / \mathrm{mol}\right)$ liberates 5.66 kJ of heat as it solidifies at its melting point. What is the mass of the sample?

How much heat is evolved when 1255 g of water condenses to a liquid at $100^{\circ} \mathrm{C}$?

What is collision theory and how does it relate to reaction rates?

Explain the difference between $K_{s p}$ and $Q_{s p}$. Is $Q_{s p}$ an equilibrium constant?

How much heat is liberated when 5.00 kg of coal is burned if the coal is 96.2% carbon by mass and the other materials in the coal do not react?

Describe how the presence of a common ion reduces the solubility of an ionic compound.