A 2.00 L container of gas has a pressure of 1.00 atm at 300 K. The temperature of the gas is halved to 150K, and the measured pressure of the same 2.00 Liter sample is 0.420 atm. Which of the following is the best explanation for these observations? A. Pressure is proportional to temperature for a fixed volume of gas. B. The molecules of the gas occupy a significant portion of the volume. C. The molecules of the gas have negligible volume of their own. D. The molecules have significant attractive forces at 150 K. E. The gas is closer to an ideal gas at 150 K.


Answer 1

The best explanation for the observation is that, the Pressure is proportional to temperature for a fixed volume of gas. (Option A)

From the question given above, the following data were obtained:

  • Initial volume (V₁) = 2 L
  • Initial pressure (P₁) = 1 atm
  • Initial temperature (T₁) = 300 K
  • Final temperature (T₂) = 150 K
  • Final volume (V₂) = 2 L = constant
  • Final pressure (P₂) = 0.420 atm

From the above, we can see that the volume is constant.

Applying the combine gas equation, we can conclude as follow:

P₁V₁ / T₁ = P₂V₂ / T₂

V₁ = V₂

P₁ / T₁ = P₂ / T₂

P/T = constant

P = constant × T

Thus, we can conclude that the pressure is proportional to the temperature at constant volume. This simply implies that the pressure will increase if the temperature increase and it will also decrease if the temperature decreases.

The correct answer to the question is Option A.

Learn more about gas laws: brainly.com/question/9631148

Answer 2






V/T -> (1)/(300)=(x)/(150)


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We have taken heat of fusion of ice = 80 cals / g

We have taken speciic heat of water = 1 cal/g per degree celsius

In this experiment ,  let the heat capacity of calorimeter be X.

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Please help!!
which oneeeee


b is the correct answer

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