N(a) The MASS of salt required is, 8.12 grams(b) The mass of the acid required is, 5.93 gramsExplanation: Given,The volume of carbon dioxide gas = 2 LThe temperature of carbon dioxide gas = 27°C = 273 + 27 = 300KThe pressure of carbon dioxide gas = 1 atmFirst, we have to calculate the moles of carbon dioxide gas by using the ideal gas equation.PV = nRTwhere,P = pressure of carbon dioxide gasV = volume of carbon dioxide gasT = temperature of carbon dioxide gasn = number of moles of carbon dioxide gasR = gas constant = 0.0821 L.atm/MOLE.K(1 atm) × (2L) = n × (0.0821 L.atm/mole.K) × (300K)n = 0.0812 mole(a) Now we have to calculate the mass of salt required.The balanced chemical reaction is,CACO3(s)+2HCl(l)⟶CaCl2(s)+H2O(l)+CO2(g)CaCOX3(s)+2HCl(l)⟶CaClX2(s)+HX2O(l)+COX2(g)From the balanced reaction, we conclude that,As, 1 mole of CO2 obtained from 1 mole of CaCO3 So, 0.0812 moles of CO2 obtained from 0.0812 moles of CaCO3Mass of CaCO3 = Moles of CaCO3 × Molar mass of CaCO3 = 0.0812 mole × 100g/mole = 8.12 gTherefore, the mass of the salt required is, 8.12 grams(b) Now we have to calculate the mass of acid required.The balanced chemical reaction is,CaCO3(s)+2HCl(l)⟶CaCl2(s)+H2O(l)+CO2(g)CaCOX3(s)+2HCl(l)⟶CaClX2(s)+HX2O(l)+COX2(g)From the balanced reaction we conclude that,As, 1 mole of CO2 obtained from 2 mole of HClSo, 0.0812 mole of CO2 obtained from 0.1624 mole of HClMass of HCl = Moles of HCl × Molar mass of HCl = 0.1624 mole × 36.5 g/mole = 5.93 gTherefore, the mass of the acid required is, 5.93 grams