Well, your "logic conclusion" got warped somehow.Bechensten said:Homework Statement
Gas occupies 2m^3 at a pressure of 100kPa. What is the pressure when the volume is 1.5m^3 and the temprature is unchanged?
Homework Equations
p=nRT/V
The Attempt at a Solution
As a logic conclusion i took 1.5/2x100 and got 75 but 175 is not the answer.. The answer is 133kPa.
I also tried the p=nRT/V.
22.4l=1mol so 1500/22.4x1 is 66.96mol. (66.96x22.4x0)/1500=0
Can someone please tell me how to calculate this type of problem?
Thank you.
Bechensten said:Homework Statement
Gas occupies 2m^3 at a pressure of 100kPa. What is the pressure when the volume is 1.5m^3 and the temprature is unchanged?
Homework Equations
p=nRT/V
The Attempt at a Solution
As a logic conclusion i took 1.5/2x100 and got 75 but 175 is not the answer.. The answer is 133kPa.
I also tried the p=nRT/V.
22.4l=1mol so 1500/22.4x1 is 66.96mol. (66.96x22.4x0)/1500=0
Can someone please tell me how to calculate this type of problem?
Thank you.
To calculate gas pressure in a variable volume, you can use the formula P = nRT/V, where P is pressure, n is the number of moles of gas, R is the gas constant, T is the temperature in Kelvin, and V is the volume.
Gas pressure is typically measured in units of Pascals (Pa), atmospheres (atm), millimeters of mercury (mmHg), or pounds per square inch (psi).
In a closed container, as the volume of gas increases, the pressure decreases. This is because the molecules have more room to move around and exert less force on the container walls.
Yes, using the ideal gas law, you can solve for pressure even if the volume is not constant. You would need to know the other variables, such as temperature, number of moles, and gas constant.
As temperature increases, gas molecules have more kinetic energy and move faster. This results in more frequent and forceful collisions with the container walls, leading to an increase in gas pressure. Similarly, as temperature decreases, gas pressure decreases.