Voltmeter Zn Salt bridge zn+ a. What is the value of E? b. What is the value of Ecell when [Zn2+] = 0.010 M and [|Cr3+] = 1.0 M? c. Based on the value of Ecell, what direction (left or right) are electrons flowing through the circuit? (If you don't know how to answer part b, how would you determine the direction?)

What is the cell potential of  Hg(l) | Hg2Cl2 | KCl(0.060 M) || KCl(0.040 M) | Cl2(0.50 bar) | Pt Select one: a. 1.094 V b. 1.774 V c. 1.166 V d. 0.128

The reduction potential to the metal of Ba 2+ is -1.57 V and that of Cu 2+ is +0.34 V.  The cell potential for the reaction  Ba(s) + Cu 2+ (aq) → Ba 2+ (aq) + Cu(s) is therefore:   a. (+1.57) + (+0.34)   b. (+1.57) + (-0.34)   c. (-1.57) + (+0.34)   d. 2 x (-1.57) + 2 x (0.34)   e. (-1.57) + (0.34)

Can someone please help with this

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.879 M and [Sn²+] = 0.0190 M. Use the standard reduction potentials in this table. Zn(s) + Sn²+ (aq) = Zn²+ (aq) + Sn(s) V I Enter numeric value TOOLS E = x10 MacBook Air

How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for 2.00 h? (F = 96,500 C/mol)

Calculate the concentration of Cu2+ Reduction potential of Zn2+(0.1 M)/Zn half-cell: –0.79 V Procedure  Pipet 1 mL of the 0.1 M Cu(NO3)2 solution (Solution 1) from the Cu2+(0.1 M)/Cu half-cell into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 2) into a 50 mL beaker. Pipet 1 mL of Solution 2 into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 3) into a 50 mL beaker. Repeat using Solution 3 to prepare Solution 4. Measure the cell potential for each of the three galvanic cells that can be made by pairing the Zn2+(0.1 M)/Zn half-cell with the half-cells containing Solutions 2–4 and the copper electrode. Make sure to rinse the copper electrode between each use

please answer a b c