An experiment using the reaction below produces 49.96 grams of chlorine gas (Cl_(2)) What mass of HF is produced by this experiment? Round your answer to the nearest 0.01 and remember to include units and substance! HCl+F_(2)... HF+Cl_(2) Your Answer: square square

## Step1: Determine the Molar Mass of Chlorine Gas<br />### Calculate the molar mass of $Cl_{2}$ using the atomic mass of chlorine (approximately 35.45 g/mol). The molar mass of $Cl_{2}$ is $2 \times 35.45 = 70.90$ g/mol.<br /><br />## Step2: Calculate Moles of Chlorine Gas Produced<br />### Use the formula $\text{moles} = \frac{\text{mass}}{\text{molar mass}}$ to find the moles of $Cl_{2}$ produced. With a mass of 49.96 grams, the moles of $Cl_{2}$ are $\frac{49.96}{70.90} \approx 0.704$ moles.<br /><br />## Step3: Use Stoichiometry to Find Moles of HF Produced<br />### According to the balanced chemical equation, 1 mole of $Cl_{2}$ is produced for every 1 mole of HF. Therefore, 0.704 moles of $Cl_{2}$ corresponds to 0.704 moles of HF.<br /><br />## Step4: Determine the Molar Mass of HF<br />### Calculate the molar mass of HF using the atomic masses of hydrogen (approximately 1.01 g/mol) and fluorine (approximately 19.00 g/mol). The molar mass of HF is $1.01 + 19.00 = 20.01$ g/mol.<br /><br />## Step5: Calculate the Mass of HF Produced<br />### Use the formula $\text{mass} = \text{moles} \times \text{molar mass}$ to find the mass of HF. The mass of HF is $0.704 \times 20.01 \approx 14.09$ grams.