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22 March, 21:41

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at 0.00°C?

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  1. 22 March, 21:53
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    1.7 atm

    Explanation:

    For first syringe:

    Pressure = 1.2 atm

    Temperature = 325 K

    Volume = 589 mL = 0.589 L (1 mL = 0.001 L)

    Using ideal gas equation as:

    PV=nRT

    where,

    P is the pressure

    V is the volume

    n is the number of moles

    T is the temperature

    R is Gas constant having value = 0.0821 L. atm/K. mol

    Applying the equation as:

    1.2 atm * 0.589 L = n * 0.0821 L. atm/K. mol * 325 K

    ⇒n = 0.02649 moles

    For second syringe:

    Pressure = 2.6 atm

    Temperature = 298 K

    Volume = 473 mL = 0.473 L (1 mL = 0.001 L)

    Using ideal gas equation as:

    PV=nRT

    Applying the equation as:

    2.6 atm * 0.473 L = n * 0.0821 L. atm/K. mol * 298 K

    ⇒n = 0.050266 moles

    Total moles = 0.02649 moles + 0.050266 moles = 0.076756 moles

    Volume = 1 L

    Temperature = 0.00 °C

    The conversion of T (°C) to T (K) is shown below:

    T (K) = T (°C) + 273.15

    So,

    T = (0 + 273.15) K = 273.15 K

    Using ideal gas equation as:

    PV=nRT

    Applying the equation as:

    P * 1 L = 0.076756 * 0.0821 L. atm/K. mol * 273.15 K

    ⇒Total P = 1.7 atm
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