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In Chemistry / High School | 2014-04-04

Propane and oxygen react according to the equation:

\[ \text{C}_3\text{H}_8(g) + 5\text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 4\text{H}_2\text{O}(g) \]

How many grams of water can be produced from the complete combustion of 2.0 moles of \(\text{C}_3\text{H}_8(g)\)?

A. 144.0
B. 82.0
C. 8.0
D. 44.8
E. 22.4

Asked by MoiraLabkovsky991

Answer (2)

1mole of propane produced 4 moles of water 44g of propane produced 18×4=72g of water 2moles of propane=2×44=88 44:72 88:x 44x=88×72 x=2×72 x=144.0grams option (a)

Answered by jydclix | 2024-06-10

The complete combustion of 2.0 moles of propane produces 8.0 moles of water, which is equivalent to 144.0 grams. Therefore, the correct option is A. 144.0 grams. This calculation is based on the stoichiometry provided in the balanced equation for the combustion of propane.
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Answered by jydclix | 2024-12-23

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