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fenix001 [56]
2 years ago
5

When hydrogen peroxide antiseptic is tightly capped and left on the shelf for a long period of time, the bottle is observed to s

well. When opened, it “hisses” noticeably. Explain these observations. Is the antiseptic likely to be as effective?
Physics
1 answer:
viktelen [127]2 years ago
5 0

Answer:

The hydrogen peroxide decomposes as: H_2O_2\rightarrow 2H_2O+O_2

Explanation:

Hydrogen peroxide antiseptic although tightly capped but left on the shelf for a long time leads to swollen bottle and opens with a hissing sound because hydrogen peroxide reacts with air in presence of light to dissociate into water and oxygen molecules that leads to high volume of content in the tightly closed bottle and formation of water molecules from hydrogen peroxide.

Once the hydrogen peroxide has turned into water molecules it is no longer effective as an antiseptic.

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Therefore, G = ΔH-TΔS

where G is Gibbs Free Energy

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Here since there is a phase change, therefore G will be 0.

∴ΔH = TΔS

Given: Temperature, T = 0°C = 273 K

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  ∴ΔH = 273 x 600

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So this is the amount of enthalpy that will be used into melting of ice.

  ∴ΔH = mass of ice melted x latent heat of fusion of water

    Mass of ice melted = ΔH / latent heat of fusion of water

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And initial amount of ice is 800 g

Amount of ice left after melting = Initial amount of ice - amount of ice melted

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                                                  = 308.109 g

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