A Question 4(1 point) Retake question A student is trying to work out how many moles of HCI are needed to produce 6.03 grams of HF according to the reaction HCl+F_(2)... HF+Cl_(2) The beginning of the student's work is shown below. What should go where the question mark is? 6.03gHFx? 20.01gHF E 1 mol HCl 1 mol HF 2 mol HF 2 mol HCI

## Step1: Determine the Molar Mass of HF<br />### Calculate the molar mass of HF using the atomic masses: Hydrogen (H) is approximately 1.01 g/mol and Fluorine (F) is approximately 19.00 g/mol. Therefore, the molar mass of HF is $1.01 + 19.00 = 20.01$ g/mol.<br />## Step2: Understand the Reaction Stoichiometry<br />### The balanced chemical equation is $HCl + F_2 \rightarrow HF + Cl_2$. This indicates a 1:1 mole ratio between HCl and HF.<br />## Step3: Set Up the Conversion Factor<br />### Since the reaction has a 1:1 mole ratio, 1 mole of HCl is needed to produce 1 mole of HF. Therefore, the conversion factor for moles of HF to moles of HCl is 1 mol HCl per 1 mol HF.