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xxTIMURxx [149]
4 years ago
5

The absolute temperature of a gas is increased four times while maintaining a constant volume. What happens to the pressure of t

he gas?
Chemistry
2 answers:
aniked [119]4 years ago
8 0

Answer:

  • <u>The pressure of a gas increases four times</u>, when <em>the absolute temperature is increased four times, while maintaining the volume constant.</em>

Explanation:

The expression that rules the change of temperature of ideal gases at constant volume is the Law of Gay-Lussac: pressure and temperature of gases are directly related. In the form of equations that is:

  • P / T = constant
  • P₁ / T₁ = P₂ / T₂ .......... [equation 1]

The question states that <em>the absolute temperature is increased four times</em>, the you can write that as T₂ = 4 × T₁, and substitute in the equation 1 to obtain:

  • P₁ / T₁ = P₂ / (4 × T₁)

Simplify:

  • P₂ = P₁ × 4 × T₁ / T₁ = P₁ × 4

That proves that the pressure also increases four times, <em>when the absolute temperature is increased four times, while maintaining the volume constant.</em>

<em></em>

scZoUnD [109]4 years ago
6 0

Answer: The pressure will also increase 4 times.

Explanation:

To calculate the final temperature of the system, we use the equation given by Gay-Lussac Law. This law states that pressure of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

\frac{P_1}{T_1}=\frac{P_2}{T_2}

where,

P_1\text{ and }T_1 are the initial pressure and temperature of the gas.

P_2\text{ and }T_2 are the final pressure and temperature of the gas.

We are given:

P_1=p\\T_1=t\\P_2=?=\\T_2=4t

Putting values in above equation, we get:

\frac{p}{t}=\frac{P_2}{4t}\\\\P_2=4p

Hence, the pressure will also increase 4 times.

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