No. For a gas, temperature also comes into the equation.
You cannot. If you know the volume, temperature and pressure of a pencil, you will be no closer to knowing its mass!
If you are given the volume, then you do not need to work it out!
The equation is P1V1=P2V2. (P1 is pressure before the change, P2 is the pressure after, V1 is the volume before the change, and V2 is the volume after it.) So to solve it, it would be the same change no matter how much the volume and pressure were to begin with. The values are P1= 1 atmosphere (the pressure of air at sea level) V1= 1 Liter which would mean P2=3 atmospheres 1*1=3(V2) 1/3 Liter= V2. So the volume would be one third of what it was before the pressure was tripled.
Gross volume is the volume at actual condition whereas standard volume is at standard Pressure/Temperature condition.
Work Done = Fs cos 0 OR- Work done by an expanding gas against a constant pressure would be w=F*d (Recall that F=PA; from P=F/A) W= (PA)d (volume = area*d) Therefore Work done = p (change in volume)
Without actually doing your homework for you ... have you noticed that if you multiply pressure by volume you get the exact units used for work?
In the relationship between volume and pressure when volume increases pressure decreases and when volume decreases pressure increases.
The volume is constant. The pressure will increase.The volume is constant. The pressure will increase.
A unit of energy such as Joules. Most often interpreted as Work assuming volume can change.
For a gas, pressure and volume are inversely related. If pressure decreases, volume will increase.
Pressure, volume, temperature & the amount of gas.
Compression reduces the volume without changing the amount of content it has. Pressure is inversely affected by volume. When volume increases, pressure decreases. Likewise, when volume decreases, pressure increases.
For a given mass at constant temperature, the pressure time tghe volume is a constant. pV=C
You cannot stretch a gas. If you extend the volume in which some gas is enclosed you are working against the difference in between the external atmospheric pressure and the internal pressure of the gas. As you increase the enclosed volume, the pressure inside there falls and you have to work harder.
"When the pressure of a gas at constant temperature is increased, the volume of the gas decreases. When the pressure is decreased, the volume increases." More precisely, pressure is inversely proportional to volume.
It would be half of the original volume. As you reduce the volume the pressure would increase and at half the original volume the pressure would be doubled.
Pressure will decrease with (because it is inversely proportianal to) volume, if (and only if!) temperature is held constant.