Answer:
1943.1 moles
Explanation:
From the question given above, the following data were obtained:
Volume (V) = 50200 L
Temperature (T) = 25 °C
Pressure (P) = 720 mmHg
Number of mole (n) of H₂ =?
Next, we shall convert 25 °C to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
Temperature (T) = 25 °C
Temperature (T) = 25 °C + 273
Temperature (T) = 298 K
Next, we shall convert 720 mmHg to atm. This can be obtained as follow:
760 mmHg = 1 atm
Therefore,
720 mmHg = 720 mmHg × 1 atm / 760 mmHg
720 mmHg = 0.947 atm
Thus, 720 mmHg is equivalent to 0.947 atm
Finally, we shall determine number of mole of Hydrogen gas, H₂, needed to fill the balloon as follow:
Volume (V) = 50200 L
Temperature (T) = 298 K
Pressure (P) = 0.947 atm
Gas constant (R) = 0.0821 atm.L/Kmol
Number of mole (n) of H₂ =?
PV = nRT
0.947 × 50200 = n × 0.0821 × 298
47539.4 = n × 24.4658
Divide both side by 24.4658
n = 47539.4 / 24.4658
n = 1943.1 moles
