Please help with the following standard reduction potentials to determine the Ksp for Hg2Cl2(s) at 25 degree celsius.
Please help with the following standard reduction potentials to determine the Ksp for Hg2Cl2(s) at 25...
Please help with the following standard reduction potentials to determine the Ksp for Hg2Cl2(s) at 25 degree celsius. 17. Given the following standard reduction potentials, E = +0.789 V Hg22 (aq) 2 Hg(%) + 2 e E = +0.271 V 2 Hg(A) 2 Cl (aq) 2 e Hg2Cl2(s) + determine Ksp for Hg2Cl2(s) at 25 °C 17. Given the following standard reduction potentials, E = +0.789 V Hg22 (aq) 2 Hg(%) + 2 e E = +0.271 V 2 Hg(A)...
please help with these, the standard reduction potentials are given in the last two pictures A standard galvanic cell is constructed in which a Cu2+ Cu half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The cathode reaction is Cu -> Cu2+ + 2e Fe2+Fe could be the other standard half cell. Hg2+Hg could be the other standard half cell. In the external...
Using the standard reduction potentials below, Hg22+(aq) + 2 e- → 2 Hg() E° = +0.789 V I2(s) + 2 e- → 2 I-(aq) E° = +0.535 V Ni2+(aq) + 2 e- → Ni(s) E° = -0.25 V (a) which element or ion is the best oxidizing agent? __________ (b) Which element or ion is the best reducing agent? __________ (c) Which element or ion will oxidize I- ions? __________
6. Use the standard reduction best oxidizing agent. potentials bdlow to determine which element or ion is the 3 E。= +0.789 V B" = +0.535 V Hig22+(aq) + 2 e-→ 2 Hg (1) Ni"(aq) + 2 e-→ Ni(s) I- (aq) Hg 1) 12(s) + 2 e→ 2 I-(aq) E°=-0.25 V d) 12(s)
Please show your work Given the following standard reduction potentials, Ag^+(aq) + e^- rightarrow Ag(s) E^degree = 0.80 V AgCN(s) + e^- rightarrow Ag(s) + CN^-(aq) E^degree = -0.01 V calculate the solubility product of AgCN at 25degree C. A) 4.3 time 10^-14 B) 2.3 times 10^13 C) 2.1 time 10^*-14 D) 5.1 times 10^13 E) None of these
Two standard reduction potentials are given below. Pb2+(aq) + 2 e− → Pb(s) E⁰red = −0.126 V Cl2(g) + 2 e− → 2 Cl−(aq) E⁰red = +1.358 V (a) Which is a stronger reducing agent, Pb(s) or Cl−(aq)? Pb(s) ; or Cl−(aq) (b) Which is the most difficult to oxidize, Pb(s) or Cl−(aq)? Pb(s); or Cl−(aq) (c) Is Pb(s) able to reduce Cl2(g) in a spontaneous reaction? is able; or is not able (d) Is Cl−(aq) able to reduce Pb2+(aq)...
Use the appropriate standard reduction potentials in the hint to calculate the value of K at 25 degree C for the reaction: 5Fe^2+ (aq) + MnO_4^- (aq) + 8H^+ (aq) rightarrow 5Fe^3+ (aq) + Mn^2+ (aq) + 4H_2O(l) K = The two half-reactions are: MnO_4^- (s) + 8H^+ (aq) + 5e^- rightarrow Mn^2+ (aq) + 4H_2O(l) E degree = 1.507V Fe^3+ (aq) + e^- rightarrow Fe^2+ (aq) E degree = 0.770V What equation relates standard reduction potentials (E degree _cell)...
#17. Electrochemistry: Consider these two entries from a fictional table of standard reduction potentials. X^2+ (aq) + 2e- --> X(s) E = 2.03 V Y^2+ (aq) + 2e- --> Y(s) E = 0.20 V Which pair of species will react under standard conditions at 25 degrees celsius? (1) X and Y (2) X^2+ and Y^2+ (3) X and Y^2+ (4) X^2+ and Y
please help the standrad reduction provided down What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 9.24x10 + M and the Cr3+ concentration is 1.47 M? 3Cu2+ (aq) + 2Cr(s) Answer: 3Cu(s) + 2Cr +(aq) v The cell reaction as written above is spontaneous for the concentrations given: What is the calculated value of the cell potential at 298K for an electrochemical cell with the...
Given the following standard reduction potentials Ag+(aq) + e- ↔ Ag(s) E = 0.80 V AgCN(s) + e- ↔ Ag(s) + CN-(aq) E = -0.01 V Calculate the solubility product of AgCN at 25°C. 4.3 &αχυτε; 10−14 2.3 &αχυτε; 1013 2.0 &αχυτε; 10−14 5.1 &αχυτε; 1013 None of the above