For this problem, we have to calculate the concentration of Pb^{2+} when the potential rose to 0.796 V

To do so, follow these steps:

**Step 1.** Determine the Cr^{2+} produced in 351 s

**Step 2.** Determine the overall reaction and find n and E°cell

**Step 3.** Use the Nernst equation to find [Pb^{2+}]

A student devises an electrochemical cell with the following cell notation:

Cr (s) | Cr^{2+} (aq, 0.02 M) | | Co^{2+} (aq, 0.9 M) | Co (s)

The student monitored the [Cr^{2+}] vs. time. The resultant data is shown in the table below.

Unfortunately, at 351 seconds, some solid Pb(NO_{3})_{2} spilled into the cathode chamber. the potential rose to 0.796 V. Determine the [Pb^{2+}] present at 351 seconds. Show all work and circle your final answer.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty of*A student devises an electrochemical cell with the following...*as high difficulty.