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Aluminium reacts with sulfuric acid to form aluminium sulfate and hydrogen. What is the volume of hydrogen gas in liters (L) produced at 300 K and 1.0 atm pressure, when 5.4 g of aluminium and 50.0 mL of 5.0 M sulfuric acid are combined for the reaction ? (Use molar mass of aluminium as 27.0 g mol–1, R = 0.082 atm L mol–1 K–1)

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answer is 6.15.

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Detailed Solution

2Al+3H2SO4⟶Al2SO43+3H2 Moles of Al takes =5.427=0.2 moles of H2SO4 taken =50×5.01000=0.25 As 0.22>0.253,H2SO4 is limiting reagent Now, moles of H2 formed =33×0.25=0.25∴ Volume of H2 gas formed =nRTP=0.25×0.082×3001=6.15L

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Aluminium reacts with sulfuric acid to form aluminium sulfate and hydrogen. What is the volume of hydrogen gas in liters (L) produced at 300 K and 1.0 atm pressure, when 5.4 g of aluminium and 50.0 mL of 5.0 M sulfuric acid are combined for the reaction ? (Use molar mass of aluminium as 27.0 g mol–1, R = 0.082 atm L mol–1 K–1)