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\(^{-1}\)].
a
6.72dm\(^3\)
b
2.24dm\(^3\)
c
0.30 dm\(^3\)
d
0.10dm\(^3\)
Explanation
Correct Option
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Discussions (4)
PrinceSeun
1 year ago
I don't think the ratio of the above equation is correct, I think it's supposed to be 4:3
