WAEC - Chemistry (2024 - No. 19)
Consider the reaction represented by the equation:
C\(_3\)H\(_8\) + 5 O\(_2\) → 3CO\(_2\) + 4H\(_2\)O
If 0.1 mole of C\(_3\)H\(_8\) was completely burnt, what volume of CO\(_2\) would be produced at stp? [volume of gas at stp = 22.4dm\(^3\)mol\(^{-1}\)].
6.72dm\(^3\)
2.24dm\(^3\)
0.30 dm\(^3\)
0.10dm\(^3\)
Explanation
C\(_3\)H\(_8\) + 5 O\(_2\) → 3CO\(_2\) + 4H\(_2\)O
From the equation: 1 mole : 3 moles
If 0.1 mole reacted, then 0.3 mole will be formed.
⇒ 0.3 mole of CO\(_2\) will be produced.
Recall that Number of moles of gases = \(\frac{Volume}{Molar Volume of gas at stp}\)
n = \(\frac{V}{M.V}\)
0.3 = \(\frac{V}{22.4}\)
V = 0.3 x 22.4
V = 6.72 dm\(^3\)
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