A 7.50g sample of aluminum is placed in 250.0 mL of 1.80 mol/L sulfuric acid.
The reaction is not nearly as vigorous as expected and produces only 427 mL of gas at 27 degrees celsius and 480 kPa pressure.
Calculate the percentage Yield of the reaction
4Al + 3H2SO4 ==> 2Al2(SO4)3 + 3H2
Does all of the Al dissolve? Assuming it does, then, how many mols H2 are produced? That's
n = PV/RT = (480*0.427)/(8.314*300) = about ?
?mols H2 x (4 mols Al/3 mols H2) = ? = grams theoretical yield.
%yield = (grams H2 produced/7.5)*100 = ?
I get about 40%.