A half-cell at a temperature of 25 \deg C produced by dissolving copper in water produces an electrode potential of +0.32 V. Calculate the amount of copper that must have been added to 1 000 mL of water to produce this potential.
Added by Sandra F.
Step 1
34 V at 25 °C. Here n = 2. Show more…
Show all steps
Your feedback will help us improve your experience
Brooke Smith and 97 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
A metal wire (M) dipped into $40 \mathrm{~mL} 1.0 \mathrm{M}$ solution of its $\mathrm{M}^{2+}$ ion has a potential of $29.5$ milli volt at $25^{\circ} \mathrm{C}$. How much volume of water be added to the metal ion solution so that when it is combined with standard hydrogen electrode, no current flows? a. $1000 \mathrm{ml}$ b. $400 \mathrm{ml}$ c. $350 \mathrm{ml}$ d. $0 \mathrm{ml}$
A student wanted to measure the copper(II) concentration in an aqueous solution. For the cathode half-cell she used a silyer electrode with a $1.00 \mathrm{M}$ solution of $\mathrm{AgNO}_{3} .$ For the anode half-cell she used a copper electrode dipped into the aqueous sample. If the cell gave $E_{\text {cell }}=0.62 \mathrm{~V}$ at $25^{\circ} \mathrm{C}$, what was the copper(II) concentration of the solution?
What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 4.9×10-6 M?
Breanna O.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD