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taurus [48]
2 years ago
15

A sample of neon gas in a bulb is at 149.05 °C and 349.84 kPa. If the pressure drops

Chemistry
1 answer:
KonstantinChe [14]2 years ago
6 0

The new temperature (in °C) of the gas, given the data is –148.20 °C

<h3>Data obtained from the question </h3>
  • Initial temperature (T₁) = 149.05 °C = 149.05 + 273 = 422.05 K
  • Initial pressure (P₁) = 349.84 KPa
  • Volume = constant
  • New pressure (P₂) = 103.45 KPa
  • New temperature (T₂) =?

<h3>How to determine the new temperature </h3>

The new temperature of the gas can be obtained by using the combined gas equation as illustrated below:

P₁V₁ / T₁ = P₂V₂ / T₂

Since the volume is constant, we have:

P₁ / T₁ = P₂ / T₂

349.84 / 422.05 = 103.45 / T₂

Cross multiply

349.84 × T₂ = 103.45 × 422.05

Divide both side by 349.84

T₂ = (103.45 × 422.05) / 349.84

T₂ = 124.80 K

Subtract 273 from 124.80 K to express in degree celsius

T₂ = 124.80 – 273

T₂ = –148.20 °C

Learn more about gas laws:

brainly.com/question/6844441

#SPJ1

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Answer:

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Explanation:

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Now, some molecules in a liquid can attain a high velocity as a random outcome of thermal motion, if this molecule is at the liquid's surface, it might actually escape! actually, many molecules might do that, and form a vapour over the liquid's surface.

Now, we know that liquids exist, therefore this process has to reach an equilibrium, that means, once the vapour becomes <em>dense </em>(or <em>concentrated</em>)<em> </em>enough, it would be as likely for a vapour molecule to re-enter the liquid as it is likely for a liquid molecule to leave the liquid and enter into the vapour.

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How can we measure how "concentrated" the vapour is? by measuring the pressure above the liquid. We know by the ideal gas law that the number of molecules in a gas is proportional to pressure at constant volume and temperature.

But how does vapour pressure relate to intermolecular forces?

Simply, the stronger the intermolecular forces, the less likely a molecule at the liquid's boundary will be to shoot of into the vapour phase! and viceversa, if intermolecular forces are very weak, the molecules won't hold together much and many molecules will leave the liquid.

As an extreme case imagine a solid, for which intermolecular forces are the strongest, what's the vapour pressure of a solid? Do solids evaporate into the air?  The answer is no, solids (with few exceptions) don't evaporate, and their vapour pressure is extremely small.

Cheers!

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The volume of the textbook calculated by the student written to 3 significant figures is 992cm³

  • According to this question, a student calculates the volume of his textbook and arrived at an answer of 991.880 cm³.

  • To round up this digit to 3 significant figures, which means that only 3 significant numbers should appear in the answer.

  • To do this, the number after the third number is 8, which means we can round up the value of 1 to 2. Hence, the volume of the textbook calculated by the student is 992cm³ in 3 s.f.

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