How Does Volume Affect Pressure
Temperature and gas calculations
Temperature can be measured using the Celsius and Kelvin scales. Gas pressure increases with temperature. Equations explain the relationship between force per unit area, temperature and volume in gases.
Book and pressure in gases – the gas laws
Boyle'southward law
Decreasing the volume of a gas increases the pressure of the gas. An instance of this is when a gas is trapped in a cylinder past a piston. If the piston is pushed in, the gas particles will have less room to move as the book the gas occupies has been decreased.
Considering the volume has decreased, the particles will collide more oft with the walls of the container. Each time they collide with the walls they exert a force on them. More collisions hateful more than force, so the pressure will increase.
When the book decreases, the pressure increases. This shows that the pressure of a gas is inversely proportional to its volume.
This is shown by the following equation - which is frequently called Boyle'southward police force . It is named after 17th century scientist Robert Boyle .
P 1 Five ane = P 2 Five two
where:
P i is the initial pressure level
V 1 is the initial volume
P 2 is the final pressure
V 2 is the final volume
It can also be written as:
pressure 1 × volume one = pressure 2 × volume 2
Note that volume is measured in metres cubed (m iii ) and pressure in pascals (Pa).
It means that for a gas at a constant temperature, pressure × book is as well constant. So increasing pressure from force per unit area 1 to pressure level two ways that volume 1 volition alter to book ii , providing the temperature remains constant.
- Question
-
A sealed syringe contains ten × ten -6 m 3 of air at one × 10 5 Pa . The plunger is pushed until the volume of trapped air is four × 10 -half dozen thou 3 . If there is no change in temperature what is the new pressure of the gas?
-
P 1 = 1 × 10 5 Pa
V 1 = 10 × ten -6 m 3
Five 2 = iv 10 ten -half dozen grand iii
P 1 V ane = P 2 5 2
Therefore:
\[p_{ii} = \frac{p_{ane}{V_{1}}}{V_{ii}}\]
\[p_{2} = \frac{{1 \times 10^{5} \times 10 \times x^{-6}}}{4 \times 10^{-half-dozen}}\]
P two = two.v × 10 v Pa
The new pressure in the syringe is 2.5 × 10 5 Pa
Charles' law
Charles' law describes the effect of irresolute temperature on the book of a gas at constant pressure. It states that:
\[volume_{1} = volume_{2} \times \frac{temperature_{i}}{temperature_{2}}\]
\[V_{ane} = V_{2} \times \frac{T_{i}}{T_{2}}\]
where:
V one is the initial volume
V 2 is the terminal volume
T 1 is the initial temperature
T 2 is the terminal temperature
Note that book is measured in metres cubed (m iii ) and temperature in kelvin (K).
This means that if a gas is heated up and the pressure does not change, the book will. So for a fixed mass of gas at a constant pressure, volume ÷ temperature remains the aforementioned.
How Does Volume Affect Pressure,
Source: https://www.bbc.co.uk/bitesize/guides/zc4xsbk/revision/3
Posted by: motenbobyth.blogspot.com
0 Response to "How Does Volume Affect Pressure"
Post a Comment