When 22.4 litres of H₂(g) is mixed with 11.2 litres of Cl₂(g), each at S.T.P., the moles of HCl(g) formed is equal to :
(a) 1 mole of HCl(g)
(b) 2 moles of HCl(g)
(c) 0.5 moles of HCl(g)
(d) 1.5 moles of HCl(g)
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Answer:
At STP, 1 mole of any gas occupies a volume of 22.4 L.
22.4lt
H
2
+
11.2lt
Cl
2
→2HCl
Limiting reagent is Cl
2
.
1 mole of chlorine forms 2 moles of HCl.
Hence, 0.5 moles of chlorine will form 1 mole of HCl.
Thus, when 22.4 liters of H
2
(g) is mixed with 11.2 liters of Cl
2
(g), each at STP, the moles of HCl(g) formed is equal to 1 mol of HCl(g).
Explanation:
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