Question

Question 2 (0.5 marks) Hydrogen gas, H2, and oxygen gas, Oz, can be reacted to form liquid water. If 2.00 g hydrogen gas and 17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in the flask at 25 "C. The vapor pressure of water is 23.8 mm Hg. Stoichiometry is involved in this question.

Answer 1

dus) find males of O2 and to a) moles of H₂ = mass = 29, =lmal molau maus b) moles of O2= b/ moes of 02 mass = 17029 = 0.5375 mol molar mass 32g/mal Stehlo bend Remalng males of exew serctent. 2 H₂(g) + O2 (g) 2H20 (1) a) mote hercofficient of H2= moles & A 2005 bl make her Coff. of Oz = 0.5375 = 005375 Hy acts as Umiding reagert. applied POAC for O moles of O2 cofficient officient - moles of O2 = 1 = 005 Step T find semaing males of Oz no = 805375 -0.5=0.0375 cofficient = 2005 72222222222 222222222222222222222 moles of H2 step w find partial pressure of Oz Po = ? no₂ = 0.0375 mol T= 25+273 = 298k 1-10

Po V = nRT PO = nRT Po, = 00375 X0.0821X 298 1.5 PO₂ = 0.612 atm ③ Napan precessure of P40 = 23.6 montly PH2O = 23.8 mntly x later 760 km Me Pro = 0.031 atm Step II, find Total pressure. P= Pro & Poz (from dalton's lane) P = 0.031+0.612 P = 0.645 atm Thank you, May it help you.