To solve this problem, we can use the combined gas equation:
(P1 * V1) / (n1 * T1) = (P2 * V2) / (n2 * T2)
Where:
P1 = initial pressure of the gas (2.0 atm)
V1 = initial volume of the gas (assuming it does not change)
n1 = initial moles of the gas (assuming it does not change)
T1 = initial temperature of the gas (8 deg C + 273.15 K)
P2 = final pressure of the gas (what we need to find)
V2 = final volume of the gas (assuming it does not change)
n2 = final moles of the gas (assuming it does not change)
T2 = final temperature of the gas (31 deg C + 273.15 K)
Plugging in the values:
(2.0 atm * V1) / (n1 * (8 + 273.15)) = (P2 * V2) / (n2 * (31 + 273.15))
Since V, n, and V2 are constant, we can simplify the equation to:
(2.0 atm) / (8 + 273.15) = P2 / (31 + 273.15)
Now, we can solve for P2:
(2.0 atm * (31 + 273.15)) / (8 + 273.15) = P2
Calculating the expression:
(2.0 atm * 304.15 K) / 281.15 K = P2
(608.3 atm·K) / 281.15 K ≈ 2.165 atm
Therefore, the pressure of the gas when it is warmed to a temperature of 31 deg C is approximately 2.17 atm.
A tank contains isoflurane, an inhaled anesthetic, at a pressure of 2.0 atm and 8 deg C
What is the pressure, in atmospheres, if the gas is warmed to a temperature of 31 deg C and if V and n do not change?
Express your answer to two significant figures and include the appropriate units
1 answer