Define the calorie. State how the calorie is related to the Calorie and the joule.

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?

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?

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?

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.

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

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

Write a balanced equation for the cell’s reaction.

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.

Suppose that you have a voltaic cell in which one half-cell is made up of a strip of tin immersed in a solution of tin (Il) ions. a. How could you tell by measuring voltage whether the tin strip was acting as a cathode or an anode in the cell? b. How could you tell by simple observation whether the tin strip was acting as a cathode or an anode?

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

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?

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.

Suppose that you have a voltaic cell in which one half-cell is made up of a strip of tin immersed in a solution of tin(II) ions. How could you tell by simple observation whether the tin strip was acting as a cathode or an anode?