Is the mass gained at the cathode the same as the mass lost at the anode? Please explain using zinc and copper
Hey
The answer to this question is NO
The mass gained would not be equal to mass lost.
Consider the example of Zn+ Cu2+------> Zn2+ + Cu
assume Zn is losing 2 electrons at a time
which means 1 Zn has converted to Zn2+
which means mass lost= mass of 1 zn=65 gram
now, moving to cathode, Copper gains the electron of Zn converting from cu2+ to Cu
which means it gained mass of 1Cu which is 63.5
so, mass lost is not equal to mass gained.
Hope it helped
Thanks!!
Is the mass gained at the cathode the same as the mass lost at the anode?...
B. Copper Electroplating 1.352 Initial Mass of Copper Anode Final Mass of Copper Anode Mass of Copper lost at Anode Moles of Copper lost at Anode Moles of Electrons produced at Anode Coulombs of Charge passed through the cell Total time current flowed (sec) Average Current (amperes) 11 3so i 00 B. Copper Electroplating minte Initial Mass of Copper Anode Final Mass of Copper Anode Mass of Copper lost at Anode Moles of Copper lost at Anode Moles of Electrons...
write oxidation and reduction (anode and cathode) reactions for given redox reactions, Write net equations as well: .1 M Cu(No3)2 added into Copper Magnesium Zinc .1 M Mg(No3)2 added into Copper Magnesium Zinc .1 M Zn(No3)2 added into Copper Magnesium Zinc Show all work please, Thank you
Draw a diagram of the electrolytic cell from Part 1. Identify the cathode, anode, directions in which the electrons, and ions move. Show how the nickel atoms migrate from the anode and how they deposit on the cathode. Show the power source and then identify the positive and negative terminals of the power source. Identify the positive and negative electrodes. Identify and write the oxidation and reduction half reactions and write the mass of each electrode at the start and...
(a) Has the rod gained or lost mass Explain O The rod has gained mass. Electrons have been added to the rod. The rod has lost mass. Electrons have been stripped from the rod (b) How much mass has the rod gained or lost? kg
need help !! with questions 2,4,5,6 Initial Mass of Cathode electrode (Fe) Initial Mass of Anode electrode (Zn) Final Mass of Cathode 10.0g 10, og 10,209 .2g Fe 3+ (aq)+32 z Fecs) Mass of Zinc deposited on cathode (g) Half reaction in Cathode Half reaction in Anode Zn(s) Eszn²+ (aq) + Ze Za(s) + 2 Fest (1) ► 2* (g) +2 Fe²+ (aq) Overall Cell Reaction Standard Cell Potential, Ecellº .440 +.763 3.32 3 (Eºcell = Ecathode - Eanode) Number...
A concentration cell is called such because both the anode and cathode are build from the same components, meaning the standard cell potential is zero volts and the measured cell potential entirely depends on the relative concentration of ions on either side of the electrochemical cell. Consider the following concentration cell Zns)lZn2() (77M)Zn2()(0.50 M)| Znø) 0.50 M) Zn Given that the concentration of zinc ions in the cathode are 0.50 M, what would the concentration of zinc ions need to...
Initial mass of the anode was 10.00 g of Zinc and the initial mass of the cathode was 10.00g of iron. A simulation was done with the current to 6.00 A and a 40.00 min time. (this information may not be needed) Part C: Electrolytic Cell and Calculation of Faraday's Constant (Using hits media.pearson me som/bc bemedia_chemchemummillest php) Cathode Final Mass 104.88 Cathode Initial Mass 16.00 4.88 Difference (m) g What do you notice in comparison to the change at...
A galvanic cell consists of a manganese anode immersed in a MnSO4 solution and a copper cathode immersed in a CuSo4 solution. A salt bridge connects the two half-cells (a) Write a balanced equation for the cell reaction. (b) A current of 1.34 A is observed to flow for a period of 1.99 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? mol (c) Calculate the change in...
The cathode has zinc can as the anode, a graphite rod in the center, surrounded by a paste of manganese dioxide, ammonium and zinc chlorides, and carbon black, is the Select one: Leclanche dry cell b Weston cell Oc. Bunsen cell od Poggendorff acid cell Daniell cell
A galvanic cell consists of a iron cathode immersed in a FeSO4 solution and a manganese anode immersed in a MnSO4 solution. A salt bridge connects the two half-cells. (a) Write a balanced equation for the cell reaction. (b) A current of 1.36 A is observed to flow for a period of 1.94 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? (c) Calculate the change in mass...