Calculate the emf of the following concentration cell: Mg(s) | Mg2+(0.35 M) || Mg2+(0.68 M) | Mg(s)
Calculate the emf of the following concentration cell: Mg(s) | Mg2+(0.35 M) || Mg2+(0.68 M) |...
Enter your answer in the provided box. Calculate the emf of the following concentration cell: Mg(s) | Mg2+(0.33 M) || Mg2+(0.68 M) | Mg(s) =_____V
Enter your answer in the provided box. Calculate the emf of the following concentration cell: Mg(s)| Mg2 (0.26 M)I| Mg2*(0.82 M) | Mg(s)
Enter your answer in the provided box. Calculate the emf of the following concentration cell: Mg(s) | Mg2+(0.22 M) || Mg2+(0.57 M) | Mg(s) V
11.) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25 C. Write the equation for the cell reaction that occurs under standard-state conditions. 12.) Calculate the emf and then predict whether the following reaction would occur spontaneously in aqueous solutions at 25 C. Assume that the initial concentrations of dissolved species are all 1.0 M. Show calculations. a.) Care) + Cd2+ (aq) → Ca2+ + Cd() b.) Br2() + Sn(3) ► 2Br...
Calculate Eº, E, and AG for the following cell reactions (a) Mg(s) + Sn2+(aq) =Mg2+(aq) + Sn(s) where [Mg2+] = 0.040 M and [Sn2+] = 0.045 M 8° = 2.23 10 E = 2.23 AG=430390 (b) 3Zn(s) + 2Cr3+(aq) = 3Zn2+(aq) + 2Cr(s) where [Cr3+] = 0.040 M and [Zn2+] = 0.0065 M E° = 0.03 E = 0.0671 AG=-0.0389
When the Cu concentration is 1.08 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.810V. What is the Mg concentration? Cu2 (aq)Mg(s) »Cu(s) + Mg2 (aq) Answer
When the Cu concentration is 1.08 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.810V. What is the Mg concentration? Cu2 (aq)Mg(s) »Cu(s) + Mg2 (aq) Answer
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 89 ∘C , where [Fe2+]= 3.50 M and [Mg2+]= 0.310 M . A. What is the value for the reaction quotient, Q, for the cell? B. What is the value for the temperature, T, in kelvins? C. What is the value for n? D. Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 87 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.110 M . A) What is the value for the reaction quotient, Q for the cell? B)What is the value for Temperature, T in Kelvins? C)What is the value for n? D) Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) (3 Significant Figures)
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 79 ∘C , where [Fe2+]= 3.80 M and [Mg2+]= 0.210 M . Part A What is the value for the reaction quotient, Q, for the cell? Part B What is the value for the temperature, T, in kelvins? Part C What is the value for n? Part D Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
Enter answer in the provided box. Calculate the emf of the following concentration cell at 25°C: Cu(s) / Cu2+(0.090 M) // Cu2+(1.645 M) / Cu(s)