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.

c. because step up transformer steps up the input voltage i.e increases the input voltage  

the number of turns are greater on the secondary side of step up transformer  

transformer does not handle dc current

it would be a gas formation