According to the collision model of chemical reactions, how is it possible that two molecules can collide but not react?

If the volume of a sample of chlorine gas is 8.2 L at 1.2 atm and 306 K, what volume will the gas occupy at STP?

Explain how the molarity of a solution is different from its molality.

What is meant by solvation? Explain how this process is important for the dissolving of ionic salts in water.

In an experimental setup, chlorine gas and nitrogen gas are in separate containers separated by a closed stopcock. One hour after the stopcock is opened, the gases have completely mixed. Five minutes after the stopcock is opened, which gas will have traveled farther, the nitrogen or the chlorine?

A battery is assembled using tin and mercury, which have the following reduction half-reactions:

$$\begin{array}{l} \mathrm{Sn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn} \\ \mathrm{Hg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg} \end{array}$$

If sodium sulfate solution is in the salt bridge, in which direction do the sulfate ions move?

A battery is assembled using tin and mercury, which have the following reduction half-reactions: $\mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}(\mathrm{aq}) \quad \mathrm{Hg}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg}(\mathrm{l})$ a. Write a balanced equation for the cell's reaction. b. What is oxidized and what is reduced? Identify the oxidizing agent and the reducing agent. c. Which reaction occurs at the anode? At the cathode? e. If sodium sulfate solution is in the salt bridge, in which direction do the sulfate ions move?

Calculate the cell potential to determine if each of the following balanced redox reactions is spontaneous as written. $2 S O_{4}^{2-}(a q)+Co^{2+}(a q) \rightarrow C o(s)+S_{2} O_{8}^{2-}(a q)$

A battery is assembled using tin and mercury, which have the following reduction half-reactions:

$$\begin{array}{l} \mathrm{Sn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn} \\ \mathrm{Hg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg} \end{array}$$

What is the cell potential?

Suppose in galvanization, copper was plated on iron instead of zinc. Would copper continue to protect the iron from corrosion, as zinc does, if the copper coating became broken or cracked? Explain.

A battery is assembled using tin and mercury, which have the following reduction half-reactions:

$$\begin{array}{l} \mathrm{Sn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn} \\ \mathrm{Hg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg} \end{array}$$

Which reaction occurs at the anode? At the cathode?

During electrolysis, an electrolytic cell releases bromine vapor and hydrogen gas. After electrolysis, the cell is found to contain a concentrated solution of potassium hydroxide. What was the composition of the cell before electrolysis began?

A battery is assembled using tin and mercury, which have the following reduction half-reactions:

$$\begin{array}{l} \mathrm{Sn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn} \\ \mathrm{Hg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg} \end{array}$$

What is oxidized and what is reduced? Identify the oxidizing agent and the reducing agent.

The potential of a half-cell varies with concentration of reactants and products. For this reason, standard potentials are measured at 1M concentration. Maintaining a pressure of 1 atm is especially important in half-cells that involve gases as reactants or products. Suggest a reason why gas pressure is critical in these cells.