To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (constant in this case)
n = number of moles (constant in this case)
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, let's convert the temperatures from degrees Celsius to Kelvin:
Initial temperature (T1) = 8 + 273.15 = 281.15 K
Final temperature (T2) = 31 + 273.15 = 304.15 K
Since volume (V) and the number of moles (n) do not change, we can rewrite the equation as:
P1/T1 = P2/T2
Now we can plug in the given values and solve for the final pressure (P2):
P1 = 2.0 atm
T1 = 281.15 K
T2 = 304.15 K
(2.0 atm)/(281.15 K) = P2/(304.15 K)
Cross-multiplying:
2.0 atm * 304.15 K = 281.15 K * P2
608.3 atm·K = 281.15 K * P2
Dividing both sides by 281.15 K:
P2 = (608.3 atm·K)/(281.15 K)
P2 ≈ 2.166 atm
Therefore, the pressure, in atmospheres, when the gas is warmed to a temperature of 31°C is approximately 2.166 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?
1 answer