When exactly of hydrogen gas () is physically mixed with of chlorine gas (), with each measured at i — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question
Question
When exactly $22.4\text{ L}$ of hydrogen gas ($H_2$) is physically mixed with $11.2\text{ L}$ of chlorine gas ($Cl_2$), with each measured at identical standard temperature and pressure (STP), what are the maximum theoretical moles of Hydrogen chloride ($HCl$) gas formed?
💡 Solution & Explanation
Step 1: Write the balanced chemical equation: $H_2(g) + Cl_2(g) \rightarrow 2HCl(g)$. Step 2: Convert volumes at STP to moles. Moles of $H_2 = 22.4 / 22.4 = 1.0\text{ mole}$. Moles of $Cl_2 = 11.2 / 22.4 = 0.5\text{ mole}$. Step 3: Identify the limiting reagent. For $H_2$: $1.0/1 = 1.0$. For $Cl_2$: $0.5/1 = 0.5$. Since $0.5 < 1.0$, Chlorine ($Cl_2$) is the limiting reagent. Step 4: Calculate product formed. $1\text{ mole}$ of $Cl_2$ yields $2\text{ moles}$ of $HCl$. Therefore, $0.5\text{ moles}$ of $Cl_2$ yields $2 \times 0.5 = 1.0\text{ mole}$ of $HCl$.