Answer:
To regulate a pressure chamber in a lab to STP (Standard Temperature and Pressure), the conditions inside the chamber need to be set to a temperature of 0 degrees Celsius (273.15 K) and a pressure of 1 atmosphere (101.325 kPa or 1013.25 hPa).
Let's assume that the three gases introduced into the pressure chamber are carbon dioxide (CO₂), nitrogen (N₂), and oxygen (O₂), and their initial quantities are as follows:
CO₂: 0.39 moles
N₂: 0.25 moles
O₂: 0.36 moles
To regulate the pressure chamber to STP, we need to calculate the total pressure of the gases inside the chamber and adjust it to 1 atmosphere if needed.
First, we need to calculate the total number of moles of gas in the chamber by summing up the moles of each gas:
Total moles of gas = moles of CO₂ + moles of N₂ + moles of O₂
Total moles of gas = 0.39 moles + 0.25 moles + 0.36 moles
Total moles of gas = 1.0 moles
Next, we can calculate the partial pressure of each gas using Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each gas:
Partial pressure of CO₂ = moles of CO₂ / total moles of gas * total pressure
Partial pressure of CO₂ = 0.39 moles / 1.0 moles * 1 atmosphere
Partial pressure of CO₂ = 0.39 atm
Partial pressure of N₂ = moles of N₂ / total moles of gas * total pressure
Partial pressure of N₂ = 0.25 moles / 1.0 moles * 1 atmosphere
Partial pressure of N₂ = 0.25 atm
Partial pressure of O₂ = moles of O₂ / total moles of gas * total pressure
Partial pressure of O₂ = 0.36 moles / 1.0 moles * 1 atmosphere
Partial pressure of O₂ = 0.36 atm
Now, we can check if the total pressure of the gases in the chamber is already at 1 atmosphere or if it needs to be adjusted.
Total pressure of gases = sum of partial pressures of each gas
Total pressure of gases = 0.39 atm + 0.25 atm + 0.36 atm
Total pressure of gases = 1.0 atm
Since the total pressure of the gases in the chamber is already 1 atmosphere, no adjustment is needed. The pressure chamber is already regulated to STP.
Step-by-step explanation: