Question

Hydrogen gas, H2, and oxygen gas, O2, 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. Total gas pressure:

Answer 1

2H₂ (g) + O₂(g) 2 H₂O (1) moles of O₂ = 17. 20g = 0.587 32.0g/mol moles of H2 = 2.0g = 1.984 1.008 g/mol = 1.984 Imole of O2 requies 2 mol of H2 - Oxygen is limiting reagent. Imolo, 2nd of Hd moles of H2O forned = 0.537X2 = 1.014 mol due to gases H₂ & O2 using where v= 1.5L PV=nRT R=0.0821 Latry/molk += 25 +273 = 298 p= nRT = (0.537 + 1.984) x 0.0821 x 298 1.5 ² 41.12 atm pdue to water = (23.8mring/760) = 0.03 atm Pt = 41. = 41.15 am