If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter?       Half-Reaction E° (V)   Zn2+(aq) + 2e– → Zn(s) –0.76     Ag+(aq) + e– → Ag(s) +0.80     Question 4 options:   a)  0.04 V   b)  2.36 V   c)  –2.36 V   d)  1.56 V   e)  –0.04 V

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Cr(s) + 3FE3+(aq)Cr3+(aq) + 3F22+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + Enter the reaction that takes place at the cathode. Include state symbols: + In the external circuit, electrons migrate v the Cr electrode v the Fe3+, Fe2+ electrode. Anions migrate v the salt bridge the Fe3+, Fe2+ compartment. Submit from proach Show Tutor Steps to

Consider the following line notation:       Cu(s)│Cu(NO3)2 (aq) (0.00678 M)║ Al(NO3)3 (aq) (0.00345M)│Al(s)         Calculate E for this electrochemical cell set up ignoring activity coefficients.  Recalculate E for the electrochemical cell with activity coefficients. (

Consider a galvanic electrochemical cell constructed using Cr/Cr³+ and Zn/Zn²+ at 25 °C. The following half-reactions are provided for each metal: Cr³+(aq) + 3 e →→ Cr(s) E°red = -0.744 V Zn²+ (aq) + 2 e →→ Zn(s) Eºred = -0.763 V Write the balanced equation for the overall reaction in acidic solution. 3 Zn(s) + 2 Cr³+ (aq) → 3 Zn²+(aq) + 2 Cr (s) 1 1 + 4- Reset 2 H₂O+ 0 3_ ( ) 3 03 04 4 H H+ 5 5 11 Zn 6 6 ²+ 7 07 (s) H₂O ● 3+ (1) 8 9 0 e 4+ x H₂O 9 (g) (aq) □o Cr Delete