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Irina-Kira [14]
2 years ago
14

A sample of gas has a volume of 100. L at 17 °C and 800. torr. To what temperature must the gas be cooled in order for its volum

e to become 50.0 L at a pressure of 600. torr? Your answer will need to be in Kelvin.
Source
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Chemistry
1 answer:
Romashka [77]2 years ago
6 0

Answer:

108.81 K

Explanation:

First convert 17 °C to Kelvin:

  • 17 + 273.16 = 290.16 K

Assuming ideal behaviour, we can solve this problem by using the<em> combined gas law</em>, which states that at constant composition:

  • P₁V₁T₂=P₂V₂T₁

Where in this case:

  • P₁ = 800 torr
  • V₁ = 100 L
  • T₂ = ?
  • P₂ = 600 torr
  • V₂ = 50 L
  • T₁ = 290.16 K

We <u>input the data</u>:

  • 800 torr * 100 L * T₂ = 600 torr * 50 L * 290.16 K

And <u>solve for T₂</u>:

  • T₂ = 108.81 K
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Answer:

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b. NaOH will dissociate, and OH will gain the proton and forms H2O as conjugate acid. pKa = 14.0, so it doesn't happen.

c. NaC≡N will dissociate, and CN will gain a proton and forms HCN as conjugate acid. pKa = 9.40, so it doesn't happen.

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We can calculate the molarity of the KBr in the final solution by dividing the total number of moles of KBr in the solution by the final volume of the solution.

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In the first sample:

Volume (V) = 35.0 mL

Concentration (C) = 1.00M

Number of moles (n) = C × V

n = (35.0mL × 1.00M)

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n = (60.0 mL × 0.600 M)

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Therefore,

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