3. At 34.0°C, the pressure inside a nitrogen-filled tennis ball with a volume of 148 cm3 is 212 kPa. How many moles of N2 are in the t

Question

3. At 34.0°C, the pressure inside a nitrogen-filled tennis ball with a volume of 148 cm3 is 212
kPa. How many moles of N2 are in the tennis ball?

in progress 0
Neala 1 year 2021-08-11T14:46:58+00:00 1 Answers 0 views 0

Answers ( )

    0
    2021-08-11T14:48:36+00:00

    Answer:

    0.0123 mol

    Explanation:

    Step 1: Convert 34.0 °C to Kelvin

    We will use the following expression.

    K = °C + 273.15 = 34.0 + 273.15 = 307.2 K

    Step 2: Convert 148 cm³ to L

    We will use the conversion factors:

    • 1 cm³ = 1 mL
    • 1 L = 1000 mL

    [tex]148cm^{3} \times \frac{1mL}{1cm^{3}} \times \frac{1L}{1000mL} = 0.148L[/tex]

    Step 3: Convert 212 kPa to atm

    We will use the conversion factor 1 atm = 101.325 kPa.

    212 kPa × 1 atm / 101.325 kPa = 2.09 atm

    Step 4: Calculate the moles of nitrogen gas

    We will use the ideal gas equation.

    P × V = n × R × T

    n = P × V / R × T

    n = 2.09 atm × 0.148 L / (0.0821 atm.L/mol.K) × 307.2 K = 0.0123 mol

Leave an answer

Browse

Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )