Answer: Option A) 240 L
Step-by-step explanation:
Given that:
Initial Volume of helium (V1) = 250.0L
Initial Temperature of helium (T1) = 22.0°C
[Convert temperature in celsius to Kelvin by adding 273
(22.0°C + 273 = 295K)]
Initial Pressure of helium (P1) = 740 mmHg
[convert pressure in mmHg to atmosphere
If 760 mmHg = 1 atm
740 mmHg = 740/760 = 0.97 atm]
Final Volume of helium (V2) = ?
Final temperature T2 = -52.0°C
[Convert -52°C to Kelvin by adding 273
-52°C + 273 = 221K]
Final pressure of helium = 0.750 atm
Since pressure, volume and temperature are given, apply the combined gas equation
(P1V1)/T1 = (P2V2)/T2
(0.97 x 250.0)/295= (0.750 x V2)/221
242.5/295 = 0.750V2/221
Cross multiply
242.5 x 221 = 0.75V2 x 295
53592.5 = 221.25V2
V2 = 53592.5 / 221.25
V2 = 242.2 L (Rounded to the nearest tens, V2 becomes 240 L)
Thus, the new volume of helium at the altitude is 240 liters