A 200 - I flask contains helium gas at a pressure of 685 torr and a temperature of 0 C what would be the pressure in the flask if the temperature is increased to 150C?
To determine the new pressure inside the flask when the temperature increases to 150°C, we can use the combined gas law. The combined gas law relates the initial and final conditions of pressure, volume, and temperature for a given amount of gas.
The combined gas law equation is:
(P1 × V1) / (T1) = (P2 × V2) / (T2)
Where:
P1 = Initial pressure
V1 = Initial volume
T1 = Initial temperature (in Kelvin)
P2 = Final pressure (unknown)
V2 = Final volume (which remains constant in this case)
T2 = Final temperature (in Kelvin)
First, let's convert the initial temperature of 0°C to Kelvin:
T1 = 0°C + 273.15 = 273.15 K
Next, we convert the final temperature of 150°C to Kelvin:
T2 = 150°C + 273.15 = 423.15 K
Since the volume (V1 = V2) remains constant, we can simplify the equation to:
P1 / T1 = P2 / T2
Now, we substitute the given values:
P1 = 685 torr
T1 = 273.15 K
T2 = 423.15 K
685 torr / 273.15 K = P2 / 423.15 K
Simplifying the equation:
P2 = (685 torr * 423.15 K) / 273.15 K
P2 = 1058.5 torr
Therefore, the pressure in the flask would be approximately 1058.5 torr when the temperature is increased to 150°C.
Answers & Comments
Answer:
What will be the new volume of 1.75L of gas that is cooled from 25°C to 0°C at constant pressure? 1.75. 298. Vz. 273. √₂ = 1160L. √2 = 5.16L.
Explanation:
Verified answer
Answer:
To determine the new pressure inside the flask when the temperature increases to 150°C, we can use the combined gas law. The combined gas law relates the initial and final conditions of pressure, volume, and temperature for a given amount of gas.
The combined gas law equation is:
(P1 × V1) / (T1) = (P2 × V2) / (T2)
Where:
P1 = Initial pressure
V1 = Initial volume
T1 = Initial temperature (in Kelvin)
P2 = Final pressure (unknown)
V2 = Final volume (which remains constant in this case)
T2 = Final temperature (in Kelvin)
First, let's convert the initial temperature of 0°C to Kelvin:
T1 = 0°C + 273.15 = 273.15 K
Next, we convert the final temperature of 150°C to Kelvin:
T2 = 150°C + 273.15 = 423.15 K
Since the volume (V1 = V2) remains constant, we can simplify the equation to:
P1 / T1 = P2 / T2
Now, we substitute the given values:
P1 = 685 torr
T1 = 273.15 K
T2 = 423.15 K
685 torr / 273.15 K = P2 / 423.15 K
Simplifying the equation:
P2 = (685 torr * 423.15 K) / 273.15 K
P2 = 1058.5 torr
Therefore, the pressure in the flask would be approximately 1058.5 torr when the temperature is increased to 150°C.
Explanation: