- Student Name Instructor Name Meso 2 Part 2 Galvanic Cells Measured E Theoretical Error Mgzn Cell Mg Cu 0 7611 1 80 1 (29.35 KiB) Viewed 110 times
- Student Name Instructor Name Meso 2 Part 2 Galvanic Cells Measured E Theoretical Error Mgzn Cell Mg Cu 0 7611 1 80 2 (52.11 KiB) Viewed 110 times
- Student Name Instructor Name Meso 2 Part 2 Galvanic Cells Measured E Theoretical Error Mgzn Cell Mg Cu 0 7611 1 80 3 (50.69 KiB) Viewed 110 times
DATA (EXP #11): Part 1: Spontaneous/Non-Spontaneous Redox Reactions Predictions: Mark as spontaneous/Non-Spontaneous based on your prediction NS NS Cu Fel Zn! Mg FeSO4 CuSO4 CuSO4 CuSO4 0.78 - 10 0,34+ = 0.78 NS 0.34 +0,707 Cu Fe/ Zn! Mg 1.10 ZnSO4 ZnSO4 FeSO FeSO. 0.33 0-33 -4.78 2.21 NS -1.93 S Cu/ MgSO4 0.34+2.43 = 3.27 Fel MgSo. Zn/ MgSO4 Mg ZnSO4 1,93 6.61 Results: Mark as "Reaction" or "No reaction" based on your observations Cu FeSO4 Fc CuSO4 Zn CuSO4 Mg CuSO4 R NR R R Cu/ ZnSO4 Zn FeSO4 Fel ZnSO4 NR Mg FeSO4 R NA ch Fel Cu/ MgSO4 Zn MgSO4 NR Mg ZnSO4 MgSO4 NR NR CHE-1261 Experiment 11
Half-Reaction E° (volts) +0.80 +0.34 0.0 Ni2+ (aq) - 0.25 2 Ag+ (aq) + 2 e → 2 Ag (5) Cu? (aq) + 2 e → Cu (8) 2 H (aq) +2e → H2 (8) +2e → Ni () (aq) + 2 c→ Fe Zn2+ (aq) + 2 e → Zn (9) Mg2+ (aq) + 2e → Mg (8) 2 K" (aq) + 2e →K 2 Li" (aq) + 2 e → Lim Fe2+ - 0.44 + I -0.76 -2.37 - 2.93 - 3.05 So, as a sort of "chain rule", if one knows the standard reduction potential of substances in reference to the standard hydrogen electrode, we can find the standard potential of their reaction with each other. For example, if we were to try to make an electrochemical cell from zinc and magnesium ions and metals... Zn + (aq) + 2e → Zn () - 0.76 Mg? (aq) +2 e → Mg - 2.37 2 CHE-1261 Experiment 11