Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and 111.1 ml of hydrogen gas over water at 26°C and 0.82 atm. (Vapor pressure of water at 26ºC = 25.2 mmHg.) How many grams of aluminum reacted?
Al reacts with water to form AlCl3 and H2 gas
2 Al(s) + 6 HCl(aq) ----------> 2 AlCl3(aq) + 3 H2(g)
2 moles of Al produces 3 moles of H2 gas
Given that, Vol. of H2 = 111.1 mL - 0.111L, Temp. = 26+273 = 299 K, Pressure = (0.82 atm - 0.033 atm) = 0.787 atm
Ideal gas equation is given by, PV=nRT
n = PV/RT = 0.787*0.111/0.0821*299 = 0.0035 moles
No. of moles of H2 gas produced = 0.0035 moles
Since, 2 moles Al = 3 moles H2
then x ? = 0.0035 moles
x = 2*0.0035/3 = 0.0023 moles of Al
Amount of Al = moles * molar mass = 0.0023*27 = 0.063 gms
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