Given the following equation:K+ underline ( )K+underline ( )Cl_(2)arrow underline ( )KCl (Balance this equation first) 4. How many grams of KCl are produced from 2.50 moles K?

## Step 1<br />The given chemical equation is \(K + Cl_2 \rightarrow KCl\). This equation is not balanced. According to the law of conservation of mass, the number of atoms of each element must be the same on both sides of the equation. Therefore, we need to balance the equation.<br /><br />## Step 2<br />To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation. In this case, we have 2 potassium atoms and 2 chlorine atoms on the left side, and 1 potassium atom and 1 chlorine atom on the right side. To balance this, we need to multiply the number of potassium and chlorine atoms on the right side by 2.<br /><br />### \(2K + Cl_2 \rightarrow 2KCl\)<br /><br />## Step 3<br />Now, we have 2 moles of potassium (K) and 2 moles of potassium chloride (KCl). The molar mass of KCl is approximately 74.5513 g/mol. Therefore, to find the mass of KCl produced, we multiply the number of moles by the molar mass.<br /><br />### \(2 \, \text{moles} \times 74.5513 \, \text{g/mol} = 149.1026 \, \text{g}\)