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mixas84 [53]
3 years ago
11

A 32 L samples of xenon gas at 10°C is expanded to 35 L. Calculate the final temperature.

Chemistry
1 answer:
morpeh [17]3 years ago
3 0

Answer:

              Final Temperature = 36.54 ⁰C

Explanation:

Lets suppose the gas is acting ideally, then according to Charle's Law, "<em>The volume of a fixed mass of gas at constant pressure is directly proportional to the absolute temperature</em>". Mathematically for initial and final states the relation is as follow,

                                                V₁ / T₁  =  V₂ / T₂

Data Given;

                  V₁  =  32 L

                  T₁  =  10 °C = 283.15 K             ∴ K = °C + 273.15

                  V₂  =  35 L

                  T₂  =  ??

Solving equation for T₂,

                         T₂  =  V₂ × T₁  / V₁

Putting values,

                         T₂  =  (35 L × 283.15 K) ÷ 32 L

                         T₂  =  309.69 K     ∴ ( 36.54 °C )

Result:

           As the volume is increased from 32 L to 35 L, therefore, the temperature must have increased from 10 °C to 36.54 °C.

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The moles of hydrogen decomposed has been given from the balanced chemical equation as:

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The moles of hydrogen decomposes has been 3.125 mol.

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Calculate the concentration of A bottle of wine contains 12.9% ethanol by volume. The density of ethanol (CH3OH) is 0.789 g/cm e
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Answer:

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The molality of the solution is 2.5403 mol/kg.

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A bottle of wine contains 12.9% ethanol by volume.

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