Question

Name Complete the following questions. Do all work on scrap paper and then neatly transfer the work onto this page. 1. A compound has the empirical formula CHCI, A 256 ml flask, at 373 K and 750 torr, contains 0.800 g of the gaseous compound. Give the molecular formula. 2. Consider two gases, A and B, each in a 1.0 L container with both gases at the same temperature and pressure. The mass of gas A in the container is 0.34 mol and the mass of gas B in the container is 0.48 mol. a) Which gas sample has the most molecules present? Show calculations. b) Which gas sample has the largest average kinetic energy? Explain.

Answer 1

P = 750 tory 1 atm = 760 torr > I torr atm V=256 me V = 0.256 L From Ideal gas equation PV = nRT eva weight x RXT T-373k GHW Weight RT P= (750) atm P = 0.987 atm → GMW= GMW = Weight = 0.89 I GHW = ? R=0.0821 Latom Knot PXV GMW = 0. 89 x 0.0821 Kathn Knot' x 3734 0.987 aliyo x 0.2564 Empirical formule weight = 12 +1+355 = 48-5 GMW = 96.96 g mo' We know that Molecular formule (MF) = 0 n= = 96.96 GMW Empirice formule weight 199 = 2 48.5 1 MF = (CHC)₂ = Ca H2 ca] Ar constant Temperature and pressure. As more no. of moles, more no. of molecules present Therefore 0.48 mol of gas 'B' has more no of moles 1 mole gas contains 6-023x102? molecules 0.34 mol = (0034 x 6.023x102, molecules lesser value 0:45 mol = (0.48 % 6:023x123) molecules - higher value No. of moles (n) < Average Kinetic energy AU.KE - ZxnxRxI is 0.48 met gas has more na kE Average ke CERT