Periodic Table Complete and balance an equation for this reaction. Al(s)+Cl_(2)(g)arrow A. 2Al(s)+2Cl_(3)(g)arrow AlCl_(3)(s) B Al(s)+Cl_(2)(g)arrow AlCl_(2)(s) C 2Al(s)+3Cl_(2)(g)arrow 2AlCl_(3)(s) D 3Al(s)+Cl_(2)(g)arrow Al_(3)Cl_(2)(s)

The question is asking for the balanced chemical equation for the reaction between aluminum (Al) and chlorine (Cl2). In a balanced chemical equation, the number of atoms of each element is the same on both sides of the equation. This is in accordance with the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.<br /><br />Option A is incorrect because the product is not correctly written. Chlorine does not exist as Cl3 in its natural state.<br /><br />Option B is incorrect because the product is not correctly written. Aluminum chloride is AlCl3, not AlCl2.<br /><br />Option C is correct. The balanced chemical equation is 2Al(s) + 3Cl2(g) → 2AlCl3(s). This means that two moles of aluminum react with three moles of chlorine to produce two moles of aluminum chloride.<br /><br />Option D is incorrect because the product is not correctly written. Aluminum chloride is AlCl3, not Al3Cl2.<br /><br />Therefore, the correct answer is option C.