What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (c) A silver wire is immersed in an aqueous solution of NiCl2.

Verified step by step guidance

1. Identify the possible redox reaction: Silver (Ag) and Nickel (Ni) can potentially undergo a redox reaction. Silver can be reduced, and nickel can be oxidized.
2. Write the half-reactions: The reduction half-reaction for silver is Ag^+ + e^- → Ag, and the oxidation half-reaction for nickel is Ni → Ni^2+ + 2e^-.
3. Determine the standard electrode potentials: Look up the standard reduction potentials for Ag^+ to Ag and Ni^2+ to Ni. Ag^+ + e^- → Ag has a potential of +0.80 V, and Ni^2+ + 2e^- → Ni has a potential of -0.25 V.
4. Calculate the cell potential: Use the formula E°_cell = E°_cathode - E°_anode. Substitute the values to find the overall cell potential.
5. Analyze the feasibility: If the calculated E°_cell is positive, the reaction is spontaneous under standard conditions. If negative, no reaction occurs.

Key Concepts

Standard-State Conditions

Standard-state conditions refer to a set of specific conditions used to measure the properties of substances. These typically include a temperature of 25°C (298 K), a pressure of 1 atm, and concentrations of 1 M for solutions. Understanding these conditions is crucial for predicting the behavior of chemical reactions and the feasibility of reactions under specified circumstances.

Electrochemical Reactions

Electrochemical reactions involve the transfer of electrons between species, often occurring in redox (reduction-oxidation) processes. In the context of the silver wire and NiCl2 solution, it is important to consider the standard reduction potentials of silver and nickel ions to determine if a spontaneous reaction can occur. The relative positions of these potentials dictate whether one metal can displace another from its ionic form.

Displacement Reactions

Displacement reactions occur when a more reactive element displaces a less reactive element from its compound. In this scenario, if silver (Ag) is more reactive than nickel (Ni) in the context of their respective ions, a reaction will take place where silver ions are produced, and nickel is deposited. Understanding the reactivity series of metals is essential for predicting the outcome of such reactions.