According to the reaction below, what mass of HCl is required to completely react with 0.76 grams of aluminum metal (Al)?Round your answer to the nearest 0.01 and remember to include units and substance! Al+HClarrow AlCl_(3)+H_(2) Your Answer: square square Answer units

## Step1: Balance the Chemical Equation<br />### The given chemical equation is unbalanced. To balance it, we need to ensure that the number of atoms for each element is equal on both sides. The balanced equation is:<br />\[ 2Al + 6HCl \rightarrow 2AlCl_3 + 3H_2 \]<br /><br />## Step2: Calculate Moles of Aluminum<br />### Use the molar mass of aluminum (Al), which is approximately 26.98 g/mol, to convert the mass of aluminum to moles.<br />\[ \text{Moles of Al} = \frac{0.76 \, \text{g}}{26.98 \, \text{g/mol}} \approx 0.0282 \, \text{mol} \]<br /><br />## Step3: Determine Moles of HCl Required<br />### According to the balanced equation, 2 moles of Al react with 6 moles of HCl. Therefore, the moles of HCl required are:<br />\[ \text{Moles of HCl} = 0.0282 \, \text{mol Al} \times \frac{6 \, \text{mol HCl}}{2 \, \text{mol Al}} = 0.0846 \, \text{mol HCl} \]<br /><br />## Step4: Convert Moles of HCl to Mass<br />### Use the molar mass of HCl, which is approximately 36.46 g/mol, to find the mass of HCl needed.<br />\[ \text{Mass of HCl} = 0.0846 \, \text{mol} \times 36.46 \, \text{g/mol} \approx 3.08 \, \text{g} \]