**xiii.** Which of the following species are reducing agents? Arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis.

K (-2.93V), Br$_2$(1.09V), Mg(-2.36V), Ce$^{3+}$(1.61V), Ti$^{2+}$(-0.37V), Ag$^+$(0.8 V)

Question

**xiii.** Which of the following species are reducing agents? Arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis.

K (-2.93V), Br$_2$(1.09V), Mg(-2.36V), Ce$^{3+}$(1.61V), Ti$^{2+}$(-0.37V), Ag$^+$(0.8 V), Ni (-0.23V).

Accepted Answer

**Step 1.** From K(-2.93V), Br2(1.09V), Mg(-2.36V), Ce3+(1.61V), Ti2+(-0.37V), Ag+(0.8V), Ni(-0.23V): the REDUCING agents are the reduced-form species capable of donating electrons -- K, Mg, Ti2+, Ni, and (weakly) Ce3+, the reduced form of the Ce4+/Ce3+ couple.
**Step 2.** Br2 and Ag+ are both OXIDISED-form species (oxidising agents), so they are excluded from the reducing-agent list. …

Element	Half-Reaction (Reduction)	$E^\ominus$ (V)
Lithium	$\text{Li}^+ + e^- \rightarrow \text{Li}$	$-3.04$
Potassium	$\text{K}^+ + e^- \rightarrow \text{K}$	$-2.93$
Calcium	$\text{Ca}^{2+} + 2e^- \rightarrow \text{Ca}$	$-2.87$
Sodium	$\text{Na}^+ + e^- \rightarrow \text{Na}$	$-2.71$
Magnesium	$\text{Mg}^{2+} + 2e^- \rightarrow \text{Mg}$	$-2.37$
Aluminium	$\text{Al}^{3+} + 3e^- \rightarrow \text{Al}$	$-1.66$
Zinc	$\text{Zn}^{2+} + 2e^- \rightarrow \text{Zn}$	$-0.76$
Iron	$\text{Fe}^{2+} + 2e^- \rightarrow \text{Fe}$	$-0.44$
Tin	$\text{Sn}^{2+} + 2e^- \rightarrow \text{Sn}$	$-0.14$
Lead	$\text{Pb}^{2+} + 2e^- \rightarrow \text{Pb}$	$-0.13$
Hydrogen	$\text{2H}^+ + 2e^- \rightarrow \text{H}_2$	$0.00$
Copper	$\text{Cu}^{2+} + 2e^- \rightarrow \text{Cu}$	$+0.34$
Silver	$\text{Ag}^+ + e^- \rightarrow \text{Ag}$	$+0.80$
Gold	$\text{Au}^{3+} + 3e^- \rightarrow \text{Au}$	$+1.50$

Q.xiii. Which of the following species are reducing agents? Arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis. K (-2.93V), Br $_2$ (1.09V), Mg(-2.36V), Ce $^{3+}$ (1.61V), Ti $^{2+}$ (-0.37V), Ag $^+$ (0.8 V), Ni (-0.23V).

Concept understanding — Electrochemical Series

The Intuition: A "Tug-of-War" for Electrons

The Precise Statement

What the Series Tells You

1. Predicting Reactivity

2. Displacement Reactions

3. Direction of Redox Reactions …

Q.xiii. Which of the following species are reducing agents? Arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis. K (-2.93V), Br2_22​(1.09V), Mg(-2.36V), Ce3+^{3+}3+(1.61V), Ti2+^{2+}2+(-0.37V), Ag+^++(0.8 V), Ni (-0.23V).

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Q.xiii. Which of the following species are reducing agents? Arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis. K (-2.93V), Br $_2$ (1.09V), Mg(-2.36V), Ce $^{3+}$ (1.61V), Ti $^{2+}$ (-0.37V), Ag $^+$ (0.8 V), Ni (-0.23V).

Unlock everything free for 14 days