To determine which compound will create an aqueous solution capable of conducting electricity, we need to identify which of these compounds can dissociate into ions when dissolved in water. Aqueous solutions that can conduct electricity typically contain ions, as they are the charge carriers.
Let's evaluate the options:
A. CH4 (methane) - This is a nonpolar molecule and does not dissociate into ions in water. It will not conduct electricity.
B. C3H7OH (propan-1-ol or isopropanol) - This is an alcohol that does not dissociate into ions, so it will not conduct electricity.
C. C6H12O6 (glucose) - This is a sugar that dissolves in water but does not produce ions. Therefore, it will not conduct electricity.
D. SrCl2 (strontium chloride) - This is an ionic compound. When dissolved in water, it dissociates into strontium ions (Sr²⁺) and chloride ions (Cl⁻). The presence of these ions in the solution will allow it to conduct electricity.
Based on this analysis, the correct answer is:
D. SrCl2