Final answer:
To determine the volume of hydrogen gas needed to react completely with 50.0 L of chlorine gas at STP, you can use the ideal gas law and stoichiometry of the reaction. 50.0 L of chlorine gas is converted to moles using the ideal gas law, and then the stoichiometry of the reaction is used to find the corresponding volume of hydrogen gas.
Step-by-step explanation:
This is a stoichiometry problem involving the reaction between hydrogen gas (H₂) and chlorine gas (Cl₂). The balanced equation for this reaction is H₂ + Cl₂ → 2HCl. From the equation, we can see that 1 mole of hydrogen reacts with 1 mole of chlorine to produce 2 moles of hydrogen chloride.
At STP (standard temperature and pressure), 1 mole of any ideal gas occupies 22.4 liters. Therefore, to determine the volume of hydrogen gas needed to react completely with 50.0 L of chlorine gas, we need to convert the volume of chlorine gas to moles and then use the stoichiometry of the reaction to find the corresponding volume of hydrogen gas.
Based on Avogadro's law, the ratio of volumes of gases in a reaction is equal to the ratio of moles of gases. So, if 50.0 L of chlorine gas is needed for the reaction, then we can calculate the moles of chlorine gas using the ideal gas law, PV = nRT, and then use the stoichiometry of the reaction to find the volume of hydrogen gas.