MI Review | Constants | Periodic Table Calculate the standard cell potential for each of the...
What is the cell potential for the reaction
Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 69 ∘C when [Fe2+]= 3.40 M and
[Mg2+]= 0.310 M . Express your answer to three significant figures
and include the appropriate units.
What is the cell potential for the reaction Mg(s) + Fe2+ (aq)+Mg2+ (aq) + Fe(s) at 69 C when Fe2+] = 3.40 Mand (Mg2+] =0.310 M. Express your answer to three significant figures and include the appropriate units. View Available Hint(s) ? com Value o D Units...
What is the cell potential for the reaction Mg(s) Fe2+ (aq)Mg2+(aq)Fe(s) at 55 °C when [Fe2+] = 3.00 Mand [Mg2+0.110 M Express your answer to three significant figures and include the appropriate units. View Available Hint(s) HA Value Units E = Submit
Consider the reaction
Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
at 69 ∘C , where [Fe2+]= 3.40 M and [Mg2+]= 0.310 M .
Constants Periodic Table Consider the reaction Mg(s) + Fe2+ (aq)+Mg2+ (aq) + Fe(s) at 69 °C, where Fe2+1 = 3.40 M and Mg²+] = 0.310 M. Part A What is the value for the reaction quotient, Q. for the cell? Express your answer numerically. ► View Available Hint(s) VO AEQ o oi ? Q= Submit Part B What is the value for the...
Consider the reaction Mg(s) + Fe^2+(aq) → Mg^2+(aq) + Fe(s) at 47 ∘C , where [Fe2+]= 3.30 M and [Mg2+]= 0.310 M . Part A: What is the value for the reaction quotient, Q, for the cell? Express your answer numerically. Part B: What is the value for the temperature, T, in kelvins? Express your answer to three significant figures and include the appropriate units. Part C: What is the value for n? Express your answer as an integer and...
What is the cell potential for the reaction Mg(s) + Fe2+ (aq)—Mg²+ (aq) + Fe(s) at 53 °C when [Fe2+] = 3.80 Mand (Mg2+] = 0.310 M. Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) E = 2.002
Consider the reaction Mg(s) + Fe2+ (aq)-Mg2+ (aq) + Fe(s) at 87 °C, where [Fe2+] = 2.80 M and [Mg2+] = 0.310 M. Part A What is the value for the reaction quotient, Q, for the cell? Express your answer numerically. ► View Available Hint(s) EVO ADV * 0 2 ? What is the value for the temperature, T, in kelvins? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) thuÀ • • •...
Consider the reaction: Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 49 ∘C , where [Fe2+]= 3.80 M and [Mg2+]= 0.310 M . Part E What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 49 ∘C when [Fe2+]= 3.80 M and [Mg2+]= 0.310 M . Express your answer to three significant figures and include the appropriate units.
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 85 ∘C , where [Fe2+]= 3.60 M and [Mg2+]= 0.210 M 1) What is the value for the reaction quotient, Q, for the cell? Express your answer numerically. 2) What is the value for the temperature, T, in kelvins? Express your answer to three significant figures and include the appropriate units. 3) What is the value for n? Express your answer as an integer and include the appropriate units (i.e. enter mol for moles). 4)...
KAssignment 18 (Chapter 18) Introduction to the Nernst Equation 1 of 3 Review I Constants Periodic Table Learning Goal: To learn how to use the Nemst equation. Consider the reaction The standard reduction potentials listed in any reference table are only valid at standard-state conditions of 25 C and 1 M, To calculate the cell potential at non-standard-state conditions, one uses the Nemst equation, Mg(s) Fe2 (aq)Mg2 (aq)Fe(s) at 43C, where Fe213.70 M and Mg2 0.310 M 2.303 RT 10g10...
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related to the standard potential, E°, by the equation Standard reduction potentials nFE RT In K E° (V) Reduction half-reaction Agt(aq)eAg(s) Cu2+(aq)2eCu(s) 0.80 where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol - K) , and T is the Kelvin temperature. 0.34 Sn4t (aq)4eSn(s) 0.15...