A 40.0 L tank of ammonia has a pressure of 8.00 atm. Calculate the volume of the ammonia if its pressure is changed to 12.0 atm while its temperature remains constant.

$1*atm$ will support a column of mercury $760$ $mm$ high. You can use a mercury column to measure a reduced pressure, or you could use a mercury bubbler as a...

First look at the things that need to be converted $35.9 ^@"C" = "(35.9 + 273.15) K" = "309.0 K"$ $"25.5 kPa = 0.2467 atm"$ $"500 mL = 0.500 L"$...

We can use the to calculate the volume. The is: $color(blue)(bar(ul(|color(white)(a/a)PV = nRTcolor(white)(a/a)|)))" "$ where $P$ is the pressure $V$ is the...

We use $"degrees Kelvin"$, and so $V_2=(P_1*V_1*T_2)/(P_2*T_1)$ $=(101.3*kPaxx2000*mLxx50*K)/(198.5*kPaxx20*K)$ $=??mL$

You can solve this problem by using Dalton's Law of Partial Pressures, which states that the of a component of a gaseous mixture depends on the mole ratio of said...

In a gaseous mixture, the exerted by a gas is the same if that gas alone had occupied the container. The total pressure is the sum of the partial pressure....

In this question Pressure and volume are given and we are asked to find out that what would be the new volume when pressure is changed from one value to...

From the information given for this question, we can see that this kind of situation is involving . Boyle's Law states that the of a fixed mass of gas...

This is an example of , which states that the volume of a given amount of a gas kept at constant temperature varies inversely with the pressure. In other words,...

So $V_2 =(P_1V_1T_2)/(P_2T_1)$ $=$ $(1.00*cancel(atm)xx2.00*L*273*cancelK)/(3.00*cancel(atm)xx323*cancelK)$ $=$ $??L$.