(c) Gold reacts with the elements in Group 7 of the periodic table. 0.175 g of gold reacts with chlorine. The equation for the reaction is: 2Au+3Cl_(2)arrow 2AuCl_(3) Calculate the mass of chlorine needed to react with 0.175 g of gold. Give your answer in mg Relative atomic masses (A); Cl=35.5Au=197

Step 1: Find the molar masses of gold (Au) and chlorine gas (Cl2).Given the relative atomic masses: Au = 197 and Cl = 35.5 However, the reaction equation involves Cl2, a chlorine molecule which contains two Cl atoms. Therefore, it's necessary to calculate the molar mass of chlorine molecule as: and the molar mass of Step 2: Identify the stoichiometry of the reaction.According to the balanced equation, This equation says that 2 moles of react with 3 moles of to form 2 moles of . Therefore, the ratio of the moles of to is .Step 3: Calculate the number of moles in 0.175g of . Step 4: Determine the number of moles of involved in the 9 * mol of . Due to the 2 to 3 stoichiometric ratio: mol( ) = mol( ) Step 5: Convert this into a mass to find the mass of chlorine needed. . Because the answer needs to be in milligrams, we just multiply by 1000 to convert. So Hence, **96 mg of Cl2 is the final result** needed to react with 0.175 g of Au according to the balanced equation.pdf