Question

Please explain to me these last two queations :(

P22. (Sec. 5.5) A 20.0 gram sample of nitrous oxide gas, N20, and a 20.0 gram sample of sulfur dioxide gas, SO2, are placed inside a 4.25 L container at temperature of 25.0°C. What are the mole fractions for each gas inside the container? Hint: Total Pressure] & (R 0.0821 L atm /mol K) a) Mole Fraction (N20) -0.593 & Mole Fraction (SO2) 0.407 Mole Fraction (N20)-0.629 & Mole Fraction (SO2) 0.371 c) Mole Fraction (N20)-0.178 & Mole Fraction (SO2)- 0.822 d) Mole Fraction (N20)-0.457 & Mole Fraction (SO2) 0.543 e) Mole Fraction (N20) 0.593& Mole Fraction (SO2)-0.783 P23. (Sec. 5.5) Zinc metal reacting with hydrochloric acid produces zinc chloride and hy gas. If hydrogen gas, H2, gas is collected over water; volume wise, how many liters of H2 gas is produced when 20 grams of sodium metal, Na, reacts at a temperature of 22.5 °C and a total pressure of 758 mm Hg? Vapor Pressure of H20 at 22.5 °C equals 20.7 mm Hg [Hint: Mole Ratio] & (R = 0.0821 L-atm / mol-K) drogen 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g) a) 5.72 L b) 21.7L c) 10.9L d) 67.3 L e) 111 L

Answer 1