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A gas has a pressure of 1.00 atm at 25 degrees Celsius. What is the pressure of the gas at 323 degrees Celsius.

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Answer:

The pressure of the gas at 323 degrees Celsius is 2 atm.

Step-by-step explanation:

Gay-Lussac's law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of collisions with the walls increases, that is, the pressure increases. That is, the pressure of the gas is directly proportional to its temperature.

In short, when there is a constant volume, as the temperature increases, the pressure of the gas increases. And when the temperature is decreased, the pressure of the gas decreases.

Gay-Lussac's law can be expressed mathematically as follows:


(P)/(T) =k

Where P = pressure, T = temperature, K = Constant

Having two different states, an initial state 1 and a final state 2, it is satisfied:


(P1)/(T1) =(P2)/(T2)

In this case:

  • P1= 1 atm
  • T1= 25 C= 298 K (being 0 C= 273 K)
  • P2= ?
  • T2= 323 C= 596 K

Replacing:


(1 atm)/(298 K) =(P2)/(596 K)

Solving:


P2=(1 atm)/(298 K)*596 K

P2= 2 atm

The pressure of the gas at 323 degrees Celsius is 2 atm.

User Volodymyr Bezuglyy
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