2C_(2)H_(3)Cl+5O_(2)arrow 4CO_(2)+ 2H_(2)O+2HCl If 24.9 liters of CO_(2) are produced at STP , how many moles of H_(2)O will also be produced?

To solve this problem, we need to use the balanced chemical equation and the given information to find the number of moles of H2O produced.Given information:- Balanced chemical equation: - Volume of CO2 produced: 24.9 liters at STPStep 1: Calculate the number of moles of CO2 produced.At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters.Number of moles of CO2 = Volume of CO2 / Volume of 1 mole of gas at STPNumber of moles of CO2 = 24.9 liters / 22.4 liters/moleNumber of moles of CO2 = 1.11 molesStep 2: Use the balanced chemical equation to find the number of moles of H2O produced.According to the balanced chemical equation, 4 moles of CO2 are produced for every 2 moles of H2O.Number of moles of H2O = (Number of moles of CO2) × (2 moles of H2O / 4 moles of CO2)Number of moles of H2O = 1.11 moles × (2 moles of H2O / 4 moles of CO2)Number of moles of H2O = 0.555 molesTherefore, if 24.9 liters of CO2 are produced at STP, 0.555 moles of H2O will also be produced.