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?

Answer 1

0.0123 mol

Step-by-step 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

`148cm^(3) * (1mL)/(1cm^(3)) * (1L)/(1000mL) = 0.148L`

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