Answer: 2169.1K
Explanation:
Given that,
Original volume of hydrogen gas (V1) = 300mL
[Convert 300mL to liters
If 1000mL = 1L
300mL = 300/1000 = 0.3L]
Original temperature of hydrogen gas (T1) = 22°C
[Convert 22°C to Kelvin by adding 273
22°C + 273 = 295K]
Original pressure of hydrogen gas = 91.9 kPa
[Since new pressure is in atm, convert 91.9 kPa to atmosphere
If 101.325 kPa = 1 atm
91.9 kPa = 91.9/101.325 = 0.9069 atm]
New volume of hydrogen gas (V2) = 2L
New temperature of hydrogen gas (T2) = ?
New pressure of hydrogen gas (P2) = 1 atm
Since pressure, volume and temperature are given, apply the formula for the combined gas equation
(P1V1)/T1 = (P2V2)/T2
(0.9069 atm x 0.3L)/295K = (1 atm x 2L)/T2
0.272 atm•L / 295K = 2 atm•L / T2
To get the value of T2, cross multiply
0.272 atm•L x T2 = 2 atm•L x 295K
0.272 atm•L•T2 = 590 atm•L•K
Divide both sides by 0.272 atm•L
0.272 atm•L•T2/0.272 atm•L = 590 atm•L•K/0.272 atm•L
T2 = 590 atm•L•K / 0.272 atm•L
T2 = 2169.1K
Thus, the new temperature of the hydrogen gas is 2169.1K
