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\nThe Ideal Gas Law\n

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\nLearn how the Ideal gas law is derived from the combined law, practice a problem and learn the difference between real and ideal gases. transcript below: ____________________________________________ Combined gas law is great! We can...\nLearn how the Ideal gas law is derived from the combined law, practice a problem and learn the difference between real and ideal gases. transcript below: ____________________________________________ Combined gas law is great! We can manipulate pressure, volume and temperature, but what about moles of the substance we’re using? Before we add moles to our equation, we need to figure out what it’s relationship is with the other variable and find out if the identity of the gas matters. because of Avogadro’s hypothesis, equal volumes of gases at the same temperature and pressure have the same number of particles. This means the identity of the gas will not matter, just the number of moles. As you increase the number of atoms in a balloon (by blowing air into the balloon) the volume increases. the pressure is the same (because the balloon can expand), the temperature is the same, so moles and volume have a direct relationship. since volume and moles are directly related just like volume and temperature are directly related we can put the number of moles, or n, next to temperature. But now we are holding nothing constant, so let’s hold one entire side constant by setting it to the STP values and call it K. and we can get rid of the division by multiplying on both sides. You don’t need the subscripts any more either. and you get Pvnrt! the ideal gas law. So much beauty in such a small mathematical equation. Let’s talk about what R is, exactly. Remember the R value is created from the equation set to STP values. So we plug in the values of pressure, the volume of a mole at STP and temperature. But remember all those pressure values? there are different R values for different pressure values, so make sure you check your problem to see which units to use. At what pressure would 0.150 mol of nitrogen gas at 23 degrees occupy 8.90 L? use pvnrt, and get pressure alone by dividing both sides by volume. now the ideal gas law makes some assumptions about ideal gases. So let’s compare ideal gases and real gases. ideal gases have no volume, but of course that isn’t the reality. real gases have volume. ideal gases have no molecular attractions, but real gases are attracted to each other. When they cool down they stop being gases and will form liquids and solids. ideal gases follow the gas laws at all pressures and temperatures, and real gases will differ at low temperatures and high pressures. So, basically there is no such thing as an ideal gas, but real gases behave like ideal gases in many conditions. This is why we can still use PV=nRT.\n
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Grade
9th - 11th
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Source:
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Date
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2015
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