NEET + JEEAdvanced
A Daniell cell operates with standard cell EMF 1.10 V at 298 K (use…
Question
A Daniell cell operates with standard cell EMF 1.10 V at 298 K (use the factor 0.0591 V for 2.303RT/F). The zinc electrode is in 0.1 M Zn2+ and the copper electrode in 0.001 M Cu2+. The cell reaction is Zn(s) + Cu2+ -> Zn2+ + Cu(s) with n = 2. Compute the cell EMF in volts, rounded to 4 decimal places.
✓ Verified answer: 1.0409checked by our engine — not a guess
Step-by-step solution
Nernst: E = E0 - (0.0591/n) log([Zn2+]/[Cu2+]). Q = 0.1/0.001 = 100, log Q = 2. E = 1.10 - (0.0591/2)(2) = 1.10 - 0.0591 = 1.0409 V. Final answer: 1.0409
Stuck on a problem like this?
Paste any JEE or NEET question — verified working, a confidence %, and an honest “not sure” instead of a bluff.
Solve my doubt →More Phys Chem Thermo Electro Kinetics solutions
For the decomposition of a solid carbonate, the standard enthalpy…NEET + JEE · PhysicsA first-order reaction is 75% complete in 60 minutes. Determine the…NEET + JEE · Physics2 moles of an ideal gas undergo isothermal reversible expansion at…NEET + JEE · PhysicsFor a reaction, the rate constant increases by a factor of 4 when…NEET + JEE · PhysicsA reaction is second order in reactant A with rate constant k = 0.05…NEET + JEE · PhysicsFor a reaction at 298 K, the standard Gibbs free energy change is…NEET + JEE · PhysicsA zero-order reaction has rate constant k = 0.02 mol/L/s and initial…NEET + JEE · PhysicsFor the ammonia synthesis reaction, the standard enthalpy change is…NEET + JEE · Physics