Calculate the standard Gibbs energy (Δ r G) for the reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). The standard electrode potential is 1.1V.

Question

Calculate the standard Gibbs energy (Δ r G) for the reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). The standard electrode potential is 1.1V., -100.15 kJ mol-1, -212.27 kJ mol-1, 55.34 kJ mol-1, 0.85 kJ mol-1

MARKS App · Accepted Answer

The standard Gibbs energy (Δ r G) can be calculated using the equation Δ r G = -nFEo, where 'n' is the number of moles of electrons transferred, 'F' is the Faraday constant(96487 C mol-1), and 'Eo' is the standard electrode potential. In this case, 'n' is 2 (since two moles of electrons are involved in the balanced reaction), and 'Eo' is 1.1 V (as provided in the information). Therefore, Δ r G ≈ -212.27 kJmol-1.

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