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### Calculate the molar mass of using the atomic mass of chlorine (approximately 35.45 g/mol). The molar mass of is g/mol.## Step2: Calculate Moles of Chlorine Gas Produced### Use the formula to find the moles of produced. With a mass of 49.96 grams, the moles of are moles.## Step3: Use Stoichiometry to Find Moles of HF Produced### According to the balanced chemical equation, 1 mole of is produced for every 1 mole of HF. Therefore, 0.704 moles of corresponds to 0.704 moles of HF.## Step4: Determine the Molar Mass of HF### 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 g/mol.## Step5: Calculate the Mass of HF Produced### Use the formula to find the mass of HF. The mass of HF is grams.