Acetylene (C2H2) burns in oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). 8.64 L of gaseous acetylene (C2H2) is burned at STP according to the equation:                            2C2H2 (g) + 5O2 (g) ⟶ 4CO2 (g) + 2H2O (l)a. What is the volume of O2 required for complete combustion?b. What is the volume of CO2 produced upon complete combustion?c. How many moles of CO2 are produced upon complete combustion?

a. To find the volume of O2 required for complete combustion, we first need to understand the stoichiometry of the reaction. According to the balanced chemical equation, 5 moles of O2 are required to completely burn 2 moles of C2H2.

Since we are given the volume of C2H2 and the conditions are at STP (Standard Temperature and Pressure), we can use Avogadro's law which states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. Therefore, the volume of a gas is directly proportional to the number of moles of the gas.

So, if 2 moles of C2H2 require 5 moles of O2, then 1 mole of C2H2 will require 5/2 = 2.5 moles of O2.

Given that the volume of C2H2 is 8.64 L, this volume represents 1 mole of C2H2 at STP. Therefore, the volume of O2 required for complete combustion is 2.5 * 8.64 L = 21.6 L.

b. According to the balanced chemical equation, 4 moles of CO2 are produced when 2 moles of C2H2 are completely burned. Therefore, 1 mole of C2H2 will produce 4/2 = 2 moles of CO2.

Given that the volume of C2H2 is 8.64 L, this volume represents 1 mole of C2H2 at STP. Therefore, the volume of CO2 produced upon complete combustion is 2 * 8.64 L = 17.28 L.

c. As mentioned in part b, 1 mole of C2H2 will produce 2 moles of CO2. Therefore, if 8.64 L of C2H2 (which is equivalent to 1 mole at STP) is completely burned, 2 moles of CO2 will be produced.