Gas, as you know, is an invaluable resource that powers everything from our cars to the furnaces that heat our homes. Without it, we're looking at a very different world.
Though for all it's value gas is also very volatile. So it stands to reason that even those of us that work with gas on a daily basis need to understand the substance down to its smallest quirks.
How it's measured, how it's used, its forms, and so on. Today, we're breaking down part of that puzzle by talking about the difference between wet gas and dry gas. The substances are very similar, though also inherently different. Natural gas is the backbone upon which we've built large swaths of society.
It heats countless homes, helps us cook food, and most importantly generates Though most people don't know the first thing about natural gas, and those that do often overlook the nuances that make it so valuable. There's a reason we're so dependent on natural gas.
Did you know that natural gas is so efficient we're now able to build a furnace that runs at 97 percent efficiency? What would the pressure be? Since the ideal gas law does not depend on which gas we have but only on the amount of any gas, the pressure of the 0. But this is just the sum of the pressure that H 2 would exert if it occupied the container alone plus the pressure of N 2 if it were the only gas present.
That is,. The pressure inside the bottle is partially from the gas being collected and partially from the water vapor that has escaped from the surface of the water in the jar. The water inside the jar will reach an equlibruim state where the number of molecules leaving the surface is the same as the number returning. The equilibrium pressure of water is temperature dependent and is called the vapor pressure of water.
Dalton's Law of Partial Pressures tells us that the total pressure in the container must be the sum of the pressures of the gas we collected and the water vapor. As the gas enters the bottle, it displaces the water and becomes trapped in the closed, upper part of the bottle.
You can use this method to measure a pure gas i. O 2 or the amount of gas produced from a reaction. The collected gas is not the only gas in the bottle, however; keep in mind that liquid water itself is always in equilibrium with its vapor phase, so the space at the top of the bottle is actually a mixture of two gases: the gas being collected, and gaseous H 2 O.
The partial pressure of H 2 O is known as the vapor pressure of water and is dependent on the temperature. To determine the quantity of gas we have collected alone, we must subtract the vapor pressure of water from the total vapor pressure of the mixture. O 2 gas is collected in a pneumatic trough with a volume of 0.
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