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

0.012 mole

Explanation:

We'll begin by converting 34.0 ℃ to Kelvin temperature. This can be obtained as follow:

T(K) = T(℃) + 273

T(℃) = 34 ℃)

T(K) = 34 + 273

T(K) = 307 K

Next, we convert 148 cm³ to L. This can be obtained as follow:

1000 cm³ = 1 L

Therefore,

148 cm³ = 148 cm³ × 1 L / 1000 cm³

148 cm³ = 0.148 L

Finally, we shall determine the number of mole of the gas. This can be obtained as follow:

Temperature (T) = 307 K

Volume (V) = 0.148 L

Pressure (P) = 212 KPa

Gas constant = 8.314 KPa.L/Kmol

Number of mole (n) =?

PV = nRT

212 × 0.148 = n × 8.314 × 307

31.376 = n × 2552.398

Divide both side by 2552.398

n = 31.376 / 2552.398

n = 0.012 mole

Thus, the number of mole of the gas in the ball is 0.012 mole.

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explanation:

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