0.41g of neon is held in a 200. mL container at 11 °C. Calculate the pressure in atm.

Question

0.41g of neon is held in a 200. mL container at 11 °C. Calculate the pressure in atm.

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niczorrrr 4 years 2021-08-14T19:02:03+00:00 1 Answers 16 views 0

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  1. Latifah
    0
    2021-08-14T19:03:48+00:00
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    Answer:

    2.39 atm

    Explanation:

    We’ll begin by calculating the number of mole in 0.41 g of neon (Ne). This can be obtained as follow:

    Mass of Ne = 0.41 g

    Molar mass of Ne = 20 g/mol

    Mole of Ne =.?

    Mole = mass / molar mass

    Mole of Ne = 0.41 / 20

    Mole of Ne = 0.0205 mole

    Next we shall convert 200 mL to L.

    1000 mL = 1 L

    Therefore,

    200 mL = 200 mL × 1 L / 1000 mL

    200 mL = 0.2 L

    Next, we shall convert 11 °C to Kelvin temperature.

    T(K) = T(°C) + 273

    T(°C) = 11 °C

    T(K) = 11 + 273

    T (K) = 284 K

    Finally, we shall determine the pressure. This can be obtained as follow:

    Mole of Ne (n) = 0.0205 mole

    Volume (V) = 0.2 L

    Temperature (T) = 284 K

    Gas constant (R) = 0.0821 atm.L/Kmol

    Pressure (P) =?

    PV = nRT

    P × 0.2 = 0.0205 × 0.0821 × 284

    P × 0.2 = 0.4779862

    Divide both side by 0.2

    P = 0.4779862 / 0.2

    P = 2.49 atm

    Therefore, the pressure of the gas is 2.39 atm

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