(a) Mg(s) + Sn2+(aq) = Mg2+(aq) + Sn(s) where [Mg2+] = 0.035 M and [Sn2+] =...
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
Calculate Eo , E, and ΔG for the following cell reaction 3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq) + 2Cr(s) where [Cr3+] = 0.090 M and [Zn2+] = 0.0085 M
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
Question 5 (1 point) Given: Cr3+(aq) + 3e --> Cr(s); E° = -0.74 V Sn2+(aq) + 2e- --> Sn(s); E° = -0.14 V What is the standard cell potential for the following reaction? 2Cr(s) + 3Sn2+(aq) --> 3Sn(s) + 2Cr3+(aq)? 0-0.60 v 0 +0.60 v O +1.06 V 0 +0.88 V 0-0.88 V
Table 20.2 Half-reaction E (V) -0.74 Cr3+ (aq) 3e --Cr (s) Fe2+(aq)+2e-Fe (s) Fe3+ (aq) 0.440 +eFe2+ (s) Sn4+ (aq) 2eSn2 (aq) +0.771 +0.154 8. Based on Table 20.2, which of the following reactions will occur spontaneously as written? A) Sn4+ (aq)+ Fe3+ (aq) Sn2+ (aq) + Fe2+ (aq) B) 3Fe (s)+2Cr3+ (aq)2Cr (s)+3F 2+ (aq) C) Sn4+ (aq)+ Fe2+ (aq) Sn2+ (aq)+ Fe (s) D) 3Sn4+ (aq)+ 2Cr (s)- 2Cr3+ (aq) + 3Sn2+ (aq) E) 3Fe2+ (aq) Fe (s)+2Fe3+...
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.
Question 2 (1 point) What is Eºcell for the cell reaction: 2Cr(s) + 3Sn4+(aq) --> 3Sn2+(aq) + 2Cr3+ (aq)? Given: Cr3+(aq) + 3e --> Cr(s); E° = -0.74 V Sn4+(aq) + 2e --> Sn2+(aq); E° = +0.15 V 0 +0.45 V O +0.89 V O 1.93 V 0-0.59 V 0 +0.59 V
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)