01 Reaction input
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02 Periodic table
6C
Carbon
Atomic number 6 · Molar mass 12.011 g/mol
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03 Molar mass & stoichiometry
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04 Electrochemistry
Cu2+ + Zn → Cu + Zn2+
E°cell = 1.10 V · n = 2 e⁻
ΔG° = -212.3 kJ mol⁻¹
E (Nernst, Q = 1) = 1.100 V
Reduction (cathode): Cu²⁺ + 2e⁻ → Cu, E° = 0.34 V. Oxidation (anode, reversed): Zn²⁺ + 2e⁻ → Zn, E° = -0.76 V. E°cell = E°cathode − E°anode = 0.34 − (-0.76) = 1.10 V. Positive, so the cell reaction is spontaneous under standard conditions.
05 Kinetics
rate = 0.001000 mol dm⁻³ s⁻¹
rate = 0.05[A][B] — overall order 2, k in dm³ mol⁻¹ s⁻¹ (k units: dm³ mol⁻¹ s⁻¹)
t½ = 100.0 s
Eₐ = 91.9 kJ mol⁻¹
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