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Q: A galvanic (voltaic) cell consists of an electrode composed of chromium in a 1.0M chromium(III) ion…

A: To calculate Standard potential , we use formula : E°cell =  E°r ( cathode ) - E°r (anode )

Q: A 215-mL sample of a 0.500 M NaCl solution with an initial pH of 7.00 is subjected to electrolysis.…

A: Gien: Volume of a sample = 215 mL NaCl = 0.500M pH = 7 After 15 minutes, Volume removed = 10 mL HCl…

Q: Chromium is electroplated from CrPO4 solution. A constant current of 13.5A is applied by an external…

A: According to the first law of Faraday, the mass of metal deposited at the anode is given by: m = E I…

Q: Sn4+ (aq) + 2e- ¬ Sn2+ (aq) +0.154 The standard cell potential (Eecell) for the voltaic cell based…

A: IMPORTANT POINTS: From net cell reaction given ,we can identify the cathode and anode of a…

Q: A steady current of 10 A maintained for 1 hr deposits 12.2 g of zinc at the cathode. What is the…

A: Given,  I = 10 A.  t = 1 hr.  m = 12.2 gm.

Q: 2. Consider the reaction MnO2(s) + 4H*(aq) + 2Br(aq) → Mn²*(aq) + Br2() + 2H2O«1) At what pH is the…

A: Given Reaction,MnO2(s) + 4Hag+ + 2 Br(aq)- → Mn(ag)2+ + Br2(l) + 2H2O(l),Write nearest equation for…

Q: OI Ag zed will a Coist A mtil 0.15 mols of metal is deposited. Which metal will require the greatest…

A: Current I is given as I= Q /t ,where Q is the charge flown in time t.  So t= Q/I

Q: Calculate the cell potential for the following electrochemical cell at 25°C. Sn(s) i Sn2+(aq, 0.022…

A: E°cell= E°(cathode)- E°(anode) [Sn^2+] = 0.022M [Ag^+] =2.7M

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: Given values:I = 0.912 ATime = 18.5 h It is known that 1 h = 3600 sec.Therefore, 18.5 h = 18.5×3600…