Question:

Pressure and volume of gas, chemistry help

by Guest64528  |  earlier

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Could someone explain these please?

A gas occupies a volume of 458 mL at a pressure of 1.01 kPa and a temperature of 295 K. When the pressure is changed, the volume becomes 477 mL. If there has been no change in temperature, what is the new pressure?

A gas occupies a volume of 2.45 L at a pressure of 1.03 atm and a temperature of 293 K. What volume will the gas occupy if the pressure changes to .980 atm and the temperature remains unchanged?

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3 ANSWERS


  1. 1)

    p1V1 = p2V2 ( Boyle's law)

    1.01 x 458 = p2 x 477

    p2 =  0.970 kPa

    2)

    1.03 x 2.45 = 0.980 V2

    V2 = 2.58 L


  2. With no temp change this is Boyle's law

    P1V1 = P2V2

    you are given three out of the four quantities so just need to calculate the remaining one. In the first question P1 = 1.01 kPa, V1 = 458 mL, and V2 = 477 mL. Solve for P2 in kPa. In the second question you need to solve for V2 in L

  3. .969kPa and 2.57 L  Pressure and volume are inverse linear relationships for ideal gas at constant temp.

    P = 1/V     P1 = 1/V1   P2 = 1/V2 therefore:  P1/P2 = (1/V1)/(1/V2)

    or P1/P2 = V2/V1     P1 = P2(V2/V1)

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