To solve this problem, we will use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature
We are given:
P = 1.00 atm
T1 = 100 °C
T2 = 145 °C
We need to find the new pressure, P2.
First, we need to convert the temperatures to Kelvin:
T1 = 100 °C + 273.15 = 373.15 K
T2 = 145 °C + 273.15 = 418.15 K
Since n and V do not change, we can write the equation as:
P1/T1 = P2/T2
Solving for P2, we have:
P2 = (P1 × T2) / T1
P2 = (1.00 atm × 418.15 K) / 373.15 K
P2 ≈ 1.122 atm
Therefore, the pressure of the steam in the autoclave when the temperature reaches 145 °C is approximately 1.122 atm.
Bacteria and viruses are inactivated by temperatures above 145 deg C in an autoclave. An autoclave contains steam at 1.00 atm and 100 deg C At what pressure, in atmospheres, will the temperature of the steam in the autoclave reach 145 deg C if n and V do not change ? Express the pressure to three significant figures and include the appropriate units.
1 answer