The number of correct statements from the following is _______
A. E$$_{cell}$$ is an intensive parameter
B. A negative E$$^\circ$$ means that the redox couple is a stronger reducing agent than the H$$^+$$/H$$_2$$ couple.
C. The amount of electricity required for oxidation or reduction depends on the stoichiometry of the electrode reaction.
D. The amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through the electrolyte.

We need to determine how many of the four statements about electrochemistry are correct.

Statement A: $$E_{\text{cell}}$$ is an intensive parameter.

This is correct. The cell potential (EMF) is an intensive property -- it does not depend on the amount of substance or the size of the cell. If you double the cell, the voltage remains the same (unlike charge or energy, which are extensive). This follows because $$E = \Delta G / (-nF)$$, where both $$\Delta G$$ and $$n$$ scale with the amount, leaving $$E$$ unchanged.

Statement B: A negative $$E^\circ$$ means the redox couple is a stronger reducing agent than the H$$^+$$/H$$_2$$ couple.

This is correct. A negative standard reduction potential means the substance is harder to reduce (or easier to oxidize) compared to H$$^+$$. The substance (in its reduced form) readily donates electrons, making it a stronger reducing agent than H$$_2$$. For example, Zn with $$E^\circ = -0.76$$ V is a stronger reducing agent than H$$_2$$.

Statement C: The amount of electricity required for oxidation or reduction depends on the stoichiometry of the electrode reaction.

This is correct. By Faraday's second law of electrolysis, the amount of electricity needed depends on the number of electrons involved in the electrode reaction. For example, reducing Cu$$^{2+}$$ requires 2 moles of electrons per mole, while reducing Ag$$^+$$ requires only 1. The stoichiometry determines the electron requirement.

Statement D: The amount of chemical reaction at any electrode during electrolysis is proportional to the quantity of electricity passed.

This is correct. This is Faraday's first law of electrolysis: $$m = \frac{MQ}{nF}$$, where $$m$$ is the mass deposited, $$Q$$ is the charge passed, $$M$$ is the molar mass, $$n$$ is the number of electrons, and $$F$$ is Faraday's constant. The mass is directly proportional to $$Q$$.

All 4 statements are correct. The answer is 4.