Which of these combinations will result in a reaction? Check all that apply. A. K(s) + Au^3+(aq) B. K^+(aq) + Au(s)

Answer: A. \( \text{K(s) + Au}^{3+}(aq) \)

Explanation:

A reaction will occur if there is a favorable redox process. In option A, solid potassium (K) is a very strong reducing agent and can easily donate electrons to reduce gold ions (\( \text{Au}^{3+} \)) to solid gold (Au). This is a spontaneous redox reaction.

In option B, potassium ions (\( \text{K}^+ \)) are already oxidized and cannot further donate electrons to reduce solid gold (Au). Therefore, no reaction will occur in this case.