Answer: 0.27L
Explanation:
Given that,
Original volume V1 = 400.0 mL
convert volume in milliliters to liters
(If 1000mL = 1L
400.0 mL = 400.0/1000 = 0.4 L)
Original temperature T1 = 22.0 °C
Convert temperature in Celsius to Kelvin
(22.0 °C + 273 = 295K)
Original pressure = 1000mmHg
Convert pressure of 1000mmHg to atm
(If 760mmHg = 1 atm
1000mmHg = 1000/760 = 1.316 atm)
New volume V2 = ?
New Temperature T2 = 30.0°C
(30.0°C + 273 = 303K)
New pressure P2 = 2 atm
Since pressure, volume and temperature are involved, apply the general gas equation
(P1V1)T1 = (P2V2)/T2
(1.316 atm x 0.4 L) /295K = (2 atm x V2) /303K
0.526 atmL / 295K = 2V2 / 303K
Cross multiply
0.526 atmL x 303K = 2V2 x 295K
159.47 = 590V2
Divide both sides by 590
159.47/590 = 590V2/590
0.27 L = V2
Thus, the final volume of the gas is 0.27L
