Under what condition is an electrochemical cell reaction spontaneous under standard state conditions?
Answer and explanation
Correct answer: A. E^\circ_cell > 0 and Delta G^\circ < 0
- Step 1: A spontaneous chemical process requires negative Gibbs free energy change: Delta G^\circ < 0. Step 2. Since Delta G^\circ = -n F E^\circ_cell, negative Delta G^\circ requires a positive standard cell potential: E^\circ_cell > 0. Answer: E^\circ_cell > 0 and Delta G^\circ < 0. Why not the others: E < 0 and Delta G > 0 characterizes non-spontaneous electrolytic cells; zeros characterize equilibrium; simultaneous positive values violate thermodynamics.
Practise more Organic Chemistry, Quantitative Analysis and Electrochemistry.
Free questions with an explanation for every one, and full timed Higher Secondary Certificate Examination (Bangladesh) mock tests.
More Organic Chemistry, Quantitative Analysis and Electrochemistry questions
- According to Markovnikov's rule, when an unsymmetrical reagent like HBr adds to Propene (CH3-CH=CH2), what is the major product?
- Under what condition does the addition of HBr to Propene yield 1-Bromopropane as the major product (anti-Markovnikov addition)? (Hard)
- What products are formed upon reductive ozonolysis (O3 followed by Zn / H2O) of 2-Butene (CH3-CH=CH-CH3)?
- Why are terminal alkynes like Ethyne (Acetylene, HC#CH) weakly acidic?
- Which reagent is used to distinguish terminal alkynes (like Propyne) from non-terminal alkynes (like 2-Butyne)?
- What is the electrophile in the nitration of benzene using a mixture of concentrated HNO3 and concentrated H2SO4? (Hard)