For the following problems identify whether the problem is a static problem (Ideal Gas Law) or a changing conditions problem (Combined Gas Law) what the value is being asked for (just the variable name) what variables names for which you have been given values (e.g., P1, T1, P2, V1, V2, etc. instead of the actual values) What will be the new pressure of air at atmospheric pressure when the volume is suddenly increased by a factor of 10? These were the 2 questions before it, if that helps at all. I have no idea I'm completely lost at this point How many moles of N2 will be contained in a 200. L cylinder that was filled to 163 atmospheres at 30 °C? If the pressure in the scuba tank of a diver in Antarctica is 900 psi at -30 °C above the ice, what will it be once he enters the water where the temperature is 0.4 °C? What will be the pressure of 2,500 moles of Argon in a 500 L cylinder at 20 °C?
For the following problems identify whether the problem is a static problem (Ideal Gas Law) or a changing conditions problem (Combined Gas Law) what the value is being asked for (just the variable name) what variables names for which you have been given values (e.g., P1, T1, P2, V1, V2, etc. instead of the actual values) What will be the new pressure of air at atmospheric pressure when the volume is suddenly increased by a factor of 10? These were the 2 questions before it, if that helps at all. I have no idea I'm completely lost at this point How many moles of N2 will be contained in a 200. L cylinder that was filled to 163 atmospheres at 30 °C? If the pressure in the scuba tank of a diver in Antarctica is 900 psi at -30 °C above the ice, what will it be once he enters the water where the temperature is 0.4 °C? What will be the pressure of 2,500 moles of Argon in a 500 L cylinder at 20 °C?
For the following problems identify whether the problem is a static problem (Ideal Gas Law) or a changing conditions problem (Combined Gas Law) what the value is being asked for (just the variable name) what variables names for which you have been given values (e.g., P1, T1, P2, V1, V2, etc. instead of the actual values) What will be the new pressure of air at atmospheric pressure when the volume is suddenly increased by a factor of 10? These were the 2 questions before it, if that helps at all. I have no idea I'm completely lost at this point How many moles of N2 will be contained in a 200. L cylinder that was filled to 163 atmospheres at 30 °C? If the pressure in the scuba tank of a diver in Antarctica is 900 psi at -30 °C above the ice, what will it be once he enters the water where the temperature is 0.4 °C? What will be the pressure of 2,500 moles of Argon in a 500 L cylinder at 20 °C?
whether the problem is a static problem (Ideal Gas Law) or a changing conditions problem (Combined Gas Law)
what the value is being asked for (just the variable name)
what variables names for which you have been given values (e.g., P1, T1, P2, V1, V2, etc. instead of the actual values)
What will be the new pressure of air at atmospheric pressure when the volume is suddenly increased by a factor of 10?
These were the 2 questions before it, if that helps at all. I have no idea I'm completely lost at this point
How many moles of N2 will be contained in a 200. L cylinder that was filled to 163 atmospheres at 30 °C?
If the pressure in the scuba tank of a diver in Antarctica is 900 psi at -30 °C above the ice, what will it be once he enters the water where the temperature is 0.4 °C?
What will be the pressure of 2,500 moles of Argon in a 500 L cylinder at 20 °C?
Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
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