For our exam preparation, our class got a review package with practice questionsHere's a question from the quot;Energy Changes and Reaction Ratesquot; unit that I can't figure out:Aluminum siding will be damaged by acid rain (sulfuric acid) due to the following reaction: 3H2SO4(aq) + 2Al(s) -gt; 3H2(g) + Al2(SO4)3 (aq)An environmental chemist reproduces this reaction in the lab by placing 13.0 g of aluminum powder in 250.0 mL of 0.15 mol/L sulfuric acid at 24 degrees CelsiusThe aluminum is consumed at an average rate of 0.0120 mol/L-s.Assuming excess acid, how long will it take for all the aluminum to fully react?^||Please help me with this question :S I don't know what to do.
That isn't much of a comparison, comparing the reaction of Al siding to Al powderNonetheless3H2SO4(aq) + 2Al(s) - 3H2(g) + Al2(SO4)3(aq) 250.0mL 13.0g 0.15M You said, 'Average rate 0.0120 mol/Ls which doesn't make a lot of senseIf you're talking about the rate of consumption of a solid, then there are no liters involved An average rate of 0.00120 mol/L per second would make sense for a substance in solution where the changes in concentration are being measuredFor a solid, it might be 0.00129 mol per second 13.0 g Al x (1 mol Al / 27.0g) x (1.00sec / 0.0120 mol Al) 40.1 seconds Follow up The average rate of 0.0120 mol/Ls must refer to the H2SO413.0 grams of Al is 0.481 molIt requires 0.722 moles of H2SO4 to completely react with the aluminum because of 3:2 mole ratio for H2SO4 to Al0.722 mol H2SO4 x (1 sec / 0.0120 mol H2SO4) 60.2 seconds ?? It also says that the aluminum is placed in 250.0 mL of 0.15 mol/L H2SO4But that is only 0.0375 moles of H2SO4, which is far less than the 0.722 moles needed to completely react with 0.480 moles of Al (13.0g)I think your question has some serious problemsIt would be a mistake to assume excess acid.
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