Final answer:
To find the new pressure of the gas after being cooled, we can use the combined gas law.
Step-by-step explanation:
In order to determine the new pressure of the gas, we can use the combined gas law which states that the ratio of the product of pressure and volume to the product of temperature and the number of moles is constant.
First, we need to convert the initial temperature and the final temperature to Kelvin by adding 273.15. So, the initial temperature is 40°C + 273.15 = 313.15K and the final temperature is 5°C + 273.15 = 278.15K.
Using the combined gas law, we can set up the equation (initial pressure)(initial volume)/(initial temperature) = (new pressure)(new volume)/(final temperature). Plugging in the values, we get (1450 mm Hg)(2 L)/(313.15 K) = (new pressure)(2 L)/(278.15 K).
Solving for the new pressure, we get new pressure = (1450 mm Hg)(278.15 K)/(313.15 K) = 1287.62 mm Hg.
To determine the new pressure of a gas that was cooled from 40°C to 5°C in a sealed 2L flask, we can use Gay-Lussac's law which relates pressure and temperature of a gas held at a constant volume. The law is stated as P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature and P2 and T2 are the final pressure and temperature, respectively.
First, we need to convert the temperatures from Celsius to Kelvin by adding 273.15. So, 40°C becomes 313.15K (40 + 273.15) and 5°C becomes 278.15K (5 + 273.15). Now, we can plug the values into the equation:
P2 = P1 * (T2/T1)
P2 = 1450 mm Hg * (278.15K/313.15K)
P2 = 1450 mm Hg * (0.888)
P2 ≈ 1287.6 mm Hg
Therefore, the new pressure will be approximately 1287.6 mm Hg after cooling.