What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (d) Hydrogen gas is bubbled through aqueous Cd(NO3)2.

Verified step by step guidance

1. Identify the components involved in the reaction: hydrogen gas (H2) and cadmium nitrate (Cd(NO3)2).
2. Determine the possible reaction: Hydrogen gas can potentially reduce cadmium ions (Cd^2+) to cadmium metal (Cd) if it is a favorable redox reaction.
3. Write the half-reactions for the reduction of Cd^2+ and the oxidation of H2: Cd^2+ + 2e^- → Cd and H2 → 2H^+ + 2e^-.
4. Use the standard reduction potentials to determine if the reaction is spontaneous: Compare the reduction potential of Cd^2+ to that of H2.
5. Conclude whether the reaction will occur by checking if the overall cell potential (E°cell) is positive, indicating a spontaneous reaction.

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 comparing thermodynamic data.

Redox Reactions

Redox reactions, or oxidation-reduction reactions, involve the transfer of electrons between species. In these reactions, one substance is oxidized (loses electrons) while another is reduced (gains electrons). Identifying the oxidation states of the reactants is essential to determine if a redox reaction occurs, such as when hydrogen gas interacts with metal ions.

Electrochemical Series

The electrochemical series is a list of standard electrode potentials for various half-reactions, which helps predict the feasibility of redox reactions. Metals higher in the series are more likely to be reduced, while those lower are more likely to be oxidized. This series is instrumental in determining whether hydrogen gas can reduce cadmium ions in the given reaction.