8. In the following reaction i) ii) iv) Zn(s) + 12(s)→→→→→→ Zn2+ (aq) + 21 (aq) Which species is being oxidized? ( Which species is being reduced? (1 Which species is the oxidizing agent? Which species is the reducing agent? 9. Consider the following equilibrium: N2(g) +202(g) + 2NO2(g) Calculate the value of the equilibrium constant if 0.0013 moles of N₂, 0.0013 mols of O₂, and 0.0028 moles of NO₂ are present in a 50mL flask at 35°C. 1

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8. In the following reaction
i)
ii)
iii)
iv)
Zn(s) + 12(s)→→→→→→ Zn²+ (aq) + 21 (aq)
-
Which species is being oxidized? ()
Which species is being reduced? (1
Which species is the oxidizing agent?
Which species is the reducing agent? (
9. Consider the following equilibrium:
N2(g) +202(g) = 2NO2(g)
Calculate the value of the equilibrium constant if 0.0013 moles of N₂, 0.0013 mols of O₂, and
0.0028 moles of NO₂ are present in a 50mL flask at 35°C. 5
Transcribed Image Text:8. In the following reaction i) ii) iii) iv) Zn(s) + 12(s)→→→→→→ Zn²+ (aq) + 21 (aq) - Which species is being oxidized? () Which species is being reduced? (1 Which species is the oxidizing agent? Which species is the reducing agent? ( 9. Consider the following equilibrium: N2(g) +202(g) = 2NO2(g) Calculate the value of the equilibrium constant if 0.0013 moles of N₂, 0.0013 mols of O₂, and 0.0028 moles of NO₂ are present in a 50mL flask at 35°C. 5
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