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The pressure of a sample of helium in a 1L container is .988 atm. What is the new pressure if the sample is placed in a 2L container?

User CrazyPyro
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1 Answer

3 votes

Answer:

The new pressure will be 0.494 atm.

Step-by-step explanation:

We can use the ideal gas law to solve this problem:

PV = nRT

where:

  • P is the pressure
  • V is the volume
  • n is the number of moles of gas
  • R is the ideal gas constant
  • T is the temperature

We know that the initial pressure is 0.988 atm, the initial volume is 1 L, and the temperature is constant.

We also know that the final volume is 2 L.

We can solve for the final pressure as follows:


P_2 = (P_1V_1)/(V_2)

substituting value


P_2 = (0.988\: atm*1 L)/(2 L)


P_2 = 0.494 atm

Therefore, the new pressure will be 0.494 atm.

User Legolas Wang
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