Pls Pls only answer if you are going to answer all of them and not just one or t

Question

Pls Pls only answer if you are going to answer all of them and not just one or two thanks i got alot in my hands cuz of finals, and don't have time to do them, Appreciate it, trust that they'll be right , I posted this once but they only did one instead of all six so yeah thanks

1) The electrochemical cell described by the balanced chemical equation has a standard emf of 0.35 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures.

2MnO42-(aq) + 2Hg2+(aq) 2MnO4-(aq) + Hg22+(aq)

2) The voltaic cell described by the balanced chemical reaction has a standard emf of 4.05 V. Calculate the equilibrium constant (Kc) for the reaction at 25 oC. Round your answer to 3 significant figures. F2(g) + Mn(s) 2F-(aq) + Mn2+(aq)

3) The voltaic cell described by the cell notation has an Eo of 0.68 V. Calculate the Wmax (kJ) the cell has done if 6.4700 mol of MnO4-(aq) (Molar Mass - 118.94 g/mol) reacts. Round your answer to 3 significant figures.

Pt(s) l VO2+(aq), VO2+(aq), H+(aq) ll H+(aq), MnO4-(aq) l MnO2(s) l Pt(s)

4) The galvanic cell described by the cell notation has an Eo of 1.23 V. Calculate the value (kJ) for the G of the cell. Round your answer to 3 significant figures.

Pt(s), H2(g) l H2O(l), OH-(aq) ll O2(g) l OH-(aq) l Pt(s)

5) The electrochemical cell described by the balanced chemical equation has a standard cell potential of -0.37 V. Calculate the value (kJ) for the standard free energy change of the cell. Round your answer to 3 significant figures.

Sn4+(aq) + 2Cu(s) Sn2+(aq) + 2Cu+(aq)

6)The electrochemical cell described by the cell notation has an Eocell of 4.05 V. Calculate the maximum electrical work (kJ) the cell has done if 375.44 g of F2(g) (Molar Mass - 38.00 g/mol) reacts. Round your answer to 3 significant figures.

Mn(s) l Mn2+(aq) ll F2(g) l F-(aq) l Pt(s)

Explanation / Answer

Ans 2- We have mass of KIO3 = 1.33 g

Molar mass of KIO3 = 39 + 126+3x16 = 214 g/mol

Volume of solution = 100 ml = 0.1 L ( 100/ 1000)

Molar concentration = moles of solute/ volume of solution in Litres

Moles of KIO3 = mass of KIO3/ Molar mass of KIO3

1.33 g/ 214 g /mol

= 0.006 Moles

Molar concentration( Molarity) = 0.006/ 0.1 = 0.06 mol/L

Ans 4 - Delta G = -nF E0cell

We have n= 2, F = 96485 C/mol, E0cell = 1.23 V

Plugging in these values, we find Delta G

Delta G = -2 x 96485 x 1.23

= 237353 J

237.353 KJ = 237 KJ ( round off to 3 sig figures)

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects