What volume of H2(g) is produced when 3.20 g of Al(s) reacts at STP?
H2(g) is produced when Al reacts with HCl.
The balanced equation between HCl and Al(s) is
2Al + 6 HCl ------------> 2AlCl3 + 3H2
2 mol 3 mol
2 x 27 g = 54 g 3 mol [ molar mass of Al = 27 g]
3.2 g ?
Then,
? = ( 3.2 g/ 54 g) x 3 mol of Al
= 0.178 mol of Al
Therefore, 0.178 moles of Al will be formed.
Now we have to calculate the volume of Al at STP.
At STP, T = 273 K , P = 1 atm
Ideal gas equation is
PV = nRT
V = nRT/P
= 0.178 mol x x 0.0821 L.atm/mol/K x 273 K / 1 atm
= 3.98 L
Volume of H2 = 3.98 L
Therefore,
volume of H2(g) is produced when 3.20 g of Al(s) reacts at STP = 3.98 L
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