1) At what pressure would a sample of gas occupy 8.96L if it occupies 3.04L at 4

Question

1) At what pressure would a sample of gas occupy 8.96L if it occupies 3.04L at 4.16atm? (Assume constant temperature)

2) A sample of gas originally occupies 26.22 L at 0C. what is its new volume when it is heated at 27C? (assume constant pressure)

3) what pressure would be required for helium at 25C to have the same density as carbon dioxide at 25C and 1.00 atm?

4) At 46C a sample of ammonia gas exerts a pressure of 4.33 atm. what is the pressure when the volume of the gas is reduced to one-third of the original value at the same temperature?

5) A gas sample occupying a volume of 24.9 mL at a pressure of 0.725 atm is allowed to expand at constant temperature until its pressure reaches 0.393 atm. what is its final volume?

(SHOW WORK) for all possible points

Explanation / Answer

1) at const T , P1/P2 = V2/V1 , P2 = P1V1/V2 = 4.16 x3.04/8.96 = 1.41 atm

2) at const T , T2/T1 = V2/V1, V2 = ( 300/273) x 26.22 = 28.813 liters ( temp is converted to Kelin )

3) d = P x Mol mass/RT , hence dHe/dCO2 = PHe x Mol mas sof He/(P CO2 x mol mass of CO2)

       since densities are equial 1 = P He x 4/( 1 x 44)

P He = 11 atm is pressure of helium required

4) T = const , (V2/V1) = 1/3 /1 = P1/P2 , hence 1/3 = 4.33/P2 , P2 = 12.99 atm

5) V2 = P1V1/P2 = 0.725 x24.9 /0.393 = 45.935 ml

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