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kakasveta [241]
3 years ago
5

Use the formation reactions below such that when added together, they match the balanced equation for the combustion of methane.

Chemistry
1 answer:
muminat3 years ago
7 0

Answer:

ΔH of the reaction is -802.3kJ.

Explanation:

Using Hess's law, you can know ΔH of reaction by the sum of ΔH's of half-reactions.

Using the reactions:

<em>(1) </em>Cgraphite(s)+ 2H₂(g) → CH₄(g) ΔH₁ = −74.80kJ

<em>(2) </em>Cgraphite(s)+ O₂(g) → CO₂(g) ΔH₂ = −393.5k J

<em>(3) </em>H₂(g) + 1/2 O₂(g) → H₂O(g) ΔH₃ = −241.80kJ

The sum of (2) - (1) produce:

CH₄(g) + O₂(g) → CO₂(g) + 2H₂(g) ΔH' = -393.5kJ - (-74.80kJ) = -318.7kJ

And the sum of this reaction with 2×(3) produce:

CH₄(g) + 2 O₂(g) → CO₂(g) + 2H₂O(g) And ΔH = -318.7kJ + 2×(-241.80kJ) =

<em>-802.3kJ</em>

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Answer:

See the explanation.

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Hydrocarbons on combustion give carbon dioxide and water.

Hydrocarbons contain all kinds of saturated and unsaturated ones.

Alkanes on reaction with oxygen gives carbon dioxide and water.

Alkenes on reaction with oxygen gives carbon dioxide and water.

Alkynes on reaction with oxygen gives carbon dioxide and water.

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These are the equations you need to learn.

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