Question

Calculate the volume of H2(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCI (g) solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. 2 HCl (g) + Mg(s) → MgCl2 (s) + H2(g) a) 0.56 L b) 4.47 L c) 2.23 L d) 1.12 L 37. What is the total pressure in atmospheres in a 10.0 L vessel containing 2.50 x 10-3 mol of H2, 1.00 x 10-3 mol of He, and 3.00 x 10-4 mol of Ne at 35.0 °C? 1.10 atm a) 2.75 x 10-2 atm b) 8.76 x 10-4 atm c) 3.80 x 10-3 atm d) 9.60 x 10-3 atm 38. A sample of natural gas contains 8.24 moles of methane, 0.421 moles of ethane, and 0.116 moles of propane. If the total pressute of the gases is 1.23 x 103 mm Hg, what is the partial pressure of ethane? a) 0.0775 atm b) 1.29 atm c) 0.0656 atm d ) 0.02 14 atm 39. Assume two cylinders at 27 °C are connected by a closed valve system. The right hand cylinder contains 3.0 L of He at 0.60 atm and the left hand cylinder contains 6.8 L of He at 2.0 atm. What is the total pressure (in atm) when the valve is opened? a) 2.6 atm b) 1.6 atm c) 24 atm d) 0.6 atm 40. a) Consider the flask diagramed below with the following pressures 492 torr for H2 and 0.376 atm for N2. What is the total pressure in torr? 868 torr b) 95.3 torr 423 torr 328 torr 2.00 LH 1.00 LN

Please answer & explain 36-40

Answer 1

3 2HCl(g) + Mg(s) → Mg 42(8) + H247). moles of HCl = molarity x volume (in. L) = 0.7257% 0.275L = 0.20mol By ran, amol HCl formsa i mole H₂ 70.20 mol HCl forms=(x0.20]arol Hy 0.10 mol H2 By Ideal gas low, PV = nRT 7 Lamm x V = 0.10 mol x 0.081 month X 273K & volume = 1.12 L (d)