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

Question

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 (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/725a29bae884bd5bf15888e70c963a0a-.png" /> H 2 SO 4 is limiting reagent ∴ Moles of H 2( g ) produced =0.25 moles Using ideal gas equation: PV = nRT ⇒ V=(0.25 × 0.082 × 300/1) V=6.15 L

H2​SO4​ is limiting reagent ∴ Moles of H2​(g) produced =0.25 moles Using ideal gas equation : PV=nRT ⇒V=10.25×0.082×300​ V=6.15L

$H_{2} S O_{4}$ is limiting reagent
$∴$ Moles of $H_{2} (g)$ produced $= 0.25$ moles
Using ideal gas equation : $P V = n RT$
$\Rightarrow V = \frac{0.25 \times 0.082 \times 300}{1}$
$V = 6.15 L$