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Chapter 20: Problem 25

Show by calculation which of the following metals will react with hydrochloric acid (standard concentrations). (a) \(\mathrm{Cd}\) (b) \(\overline{\mathrm{Cr}}\) (c) Co (d) \(\mathrm{Ag}\) (c) Au

Short Answer

Expert verified
Answer: Ag and Au will react with hydrochloric acid.

Step by step solution

01

Find the standard electrode potentials of each metal

Look up the standard electrode potentials of each metal: \(\mathrm{Cd}\), \(\overline{\mathrm{Cr}}\), Co, \(\mathrm{Ag}\), and Au in a reference source or a textbook. These values are usually represented as half-cell reactions, with the metal reducing and the metal ion being oxidized.
02

Identify the half-cell reaction for H\(^+\) ions in hydrochloric acid

The hydrogen ions (H\(^+\)) in hydrochloric acid can be reduced to form hydrogen gas. The half-cell reaction for this is: \(2\mathrm{H^+} + 2\mathrm{e^-} \rightarrow \mathrm{H_2}\) The standard electrode potential for this half-cell reaction is 0 V.
03

Determine the feasibility of redox reactions

In order for a reaction between the metal and hydrochloric acid to occur, the overall cell potential must be greater than zero. The cell potential can be calculated using the formula: E\(_{cell}\) = E\(_{cathode}\) - E\(_{anode}\) As the half-cell reaction involving H\(^+\) ions has a potential of 0 V, the cell potential will be equal to the standard electrode potential of the metal half-cell. If the metal half-cell potential is greater than 0 V, the reaction will be feasible and the metal will react with the hydrochloric acid.
04

Compare each metal's standard electrode potential to 0 V

Based on the standard electrode potentials you found in Step 1, compare each metal's potential to 0 V. If the metal's potential is greater than 0 V, it will react with hydrochloric acid. Note: The values provided below are examples and may differ depending on the reference source. \(\mathrm{Cd:}\) E\(^\circ\) = -0.40 V (Less than 0 V; will not react) \(\overline{\mathrm{Cr}}\) E\(^\circ\) = -0.74 V (Less than 0 V; will not react) Co E\(^\circ\) = -0.28 V (Less than 0 V; will not react) \(\mathrm{Ag:}\) E\(^\circ\) = +0.80 V (Greater than 0 V; will react) Au E\(^\circ\) = +1.50 V (Greater than 0 V; will react)
05

Report the metals that will react with hydrochloric acid

Based on the comparison of standard electrode potentials, only \(\mathrm{Ag}\) and Au will react with hydrochloric acid (as their potentials are greater than 0 V).

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