NEETChemistryElectrochemistry
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.
Options
- A-100.15 kJ mol-1
- B-212.27 kJ mol-1
- C55.34 kJ mol-1
- D0.85 kJ mol-1
Correct answer
B. -212.27 kJ mol-1
Step-by-step solution
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.