15) On a cold day, you take in 4.2 L (i.e., 4.2 x 10-3 m3) of air into your lungs at a temperature of 0°C. If you hold your breath until the

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15) On a cold day, you take in 4.2 L (i.e., 4.2 x 10-3 m3) of air into your lungs at a temperature of 0°C. If you hold your breath until the temperature of the air in your lungs reaches 37°C, what is the volume of the air in your lungs at that point, assuming the pressure does not change?

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RuslanHeatt 2 weeks 2021-07-20T04:56:11+00:00 1 Answers 8 views 0

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    2021-07-20T04:57:39+00:00

    Answer:

    4.8L ( i.e 4.8 x 10^-3 m3)

    Explanation:

    Step 1:

    Data obtained from the question.

    Initial volume (V1) = 4.2L

    Initial temperature (T1) = 0°C

    Final temperature (T2) = 37°C

    Final volume (V2) =?

    Step 2:

    Conversion of celsius temperature to Kelvin temperature. This is illustrated below

    K = °C + 273

    T1 = 0°C = 0°C + 273 = 273K

    T2 = 37°C = 37°C + 273 = 310K

    Step 3:

    Determination of the final volume.

    Since the pressure is constant,

    Charles’ Law equation will be applied as shown below:

    V1 /T1 = V2/T2

    4.2/273 = V2 /310

    Cross multiply to express in linear form

    273 x V2 = 4.2 x 310

    Divide both side by 273

    V2 = (4.2 x 310)/273

    V2 = 4.8L ( i.e 4.8 x 10^-3 m3)

    Therefore, the volume of the air in the lungs at that point is 4.8L ( i.e 4.8 x 10^-3 m3)

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