Background Infromation
We use gas laws everyday. Whether it is changing tire pressure in your car in the winter, making sure balloons don't pop in the summer, or like the scuba diver on the home page the pressure in your oxygen tank, just to name a few.
The relationship between pressure, temperature, and volume of gases have been studied since the 1600s. Scientists everywhere found similar relationships but the ones we are going to focus on are Boyle's Law, Charles's Law, Gay-Lussac's Law, Combined Gas Law, and Ideal gas law.
Before discussing these gas laws, I would like to take the time to explain what units we will be using in class and in these equations. For pressure, we will use: atmospheres (atm), torr, or mmHg and conversions of each I will provide. Volume we will measure in mL or Liters. And temperature we will measure in Kelvin or Celcius. Now since you have units in mind, we are going to briefly explain each law below.
Boyle's Law closely looks at the relationship of volume and pressure in the form of p1v1=p2v2. The 1 means the initial state and 2 means the final state in any equation we use in class. Temperature is not a factor in this equation. As a result of organizing the equation in this manner, pressure and volume are inversely proportional. As pressure increases, volume decreases. An example of Boyle's Law would be changing pressure in a syringe or popping a balloon.
Charles's Law closely looks at the relationship between volume and temperature in the form of v1/t1=v2/t2. In this case, pressure is constant while volume temperature may experience change. As a result, volume and temperature are proportionally related. As in the temperature increases, the volume of the gas will also increase. An example of Charles's Law is a hot air balloon, and I will discuss the reasons why with a diagram in class.
Gay-Lussac's Law examines the relationship between pressure and temperature in the form p1/t1=p2/t2. In this case, volume of gas is kept constant. Like Charles's Law, pressure and temperature are proportionally related. As temperature increases, temperature increases. An example of Gay-Lussac's Law is When the can is cold, is fizzes less when you open it because there is less pressure. When you have a warm soda can, it fizzes more because there is more pressure.
The Combined Gas Law combines Boyle's Law, Charles's Law, and Gay-Lussac's Law in the equation: p1v1/t1=p2v2/t2. This is an equation I will explain more in detail in class. It is very important to understand how each of these variables interact and we will go into specific examples in class.
The last law we are going to discuss in this class is the Ideal Gas Law. The formula and conditions for this Law are: pv=nrt and STP. n stands for the number of moles of gas, p is pressure, v is volume, r is a constant, and t is temperature. STP stands for standard temperature and pressure, which is 0 atm and 273 Kelvin. These conditions are when gases are "ideal." Obviously, gases do not always exist in these conditions, and therefore we can discuss trends associated with this equation.
I have attached a worksheet that we will complete in class to explain what each mean and which relationship they represent. The most important thing to remember in that the Ideal Gas Law takes into account the amount of Moles of a gas that is present and can only be used for ideal gases, which has several limitations that we will talk about in class.
I have also attached a link that has a general definition of what each law's relationship is. Please feel free to look around this website and familiarize yourself with the concepts and examples (Hint: a question on your next test may include a concept from this website). http://legacyweb.chemistry.ohio-state.edu/betha/nealGasLaw/
The relationship between pressure, temperature, and volume of gases have been studied since the 1600s. Scientists everywhere found similar relationships but the ones we are going to focus on are Boyle's Law, Charles's Law, Gay-Lussac's Law, Combined Gas Law, and Ideal gas law.
Before discussing these gas laws, I would like to take the time to explain what units we will be using in class and in these equations. For pressure, we will use: atmospheres (atm), torr, or mmHg and conversions of each I will provide. Volume we will measure in mL or Liters. And temperature we will measure in Kelvin or Celcius. Now since you have units in mind, we are going to briefly explain each law below.
Boyle's Law closely looks at the relationship of volume and pressure in the form of p1v1=p2v2. The 1 means the initial state and 2 means the final state in any equation we use in class. Temperature is not a factor in this equation. As a result of organizing the equation in this manner, pressure and volume are inversely proportional. As pressure increases, volume decreases. An example of Boyle's Law would be changing pressure in a syringe or popping a balloon.
Charles's Law closely looks at the relationship between volume and temperature in the form of v1/t1=v2/t2. In this case, pressure is constant while volume temperature may experience change. As a result, volume and temperature are proportionally related. As in the temperature increases, the volume of the gas will also increase. An example of Charles's Law is a hot air balloon, and I will discuss the reasons why with a diagram in class.
Gay-Lussac's Law examines the relationship between pressure and temperature in the form p1/t1=p2/t2. In this case, volume of gas is kept constant. Like Charles's Law, pressure and temperature are proportionally related. As temperature increases, temperature increases. An example of Gay-Lussac's Law is When the can is cold, is fizzes less when you open it because there is less pressure. When you have a warm soda can, it fizzes more because there is more pressure.
The Combined Gas Law combines Boyle's Law, Charles's Law, and Gay-Lussac's Law in the equation: p1v1/t1=p2v2/t2. This is an equation I will explain more in detail in class. It is very important to understand how each of these variables interact and we will go into specific examples in class.
The last law we are going to discuss in this class is the Ideal Gas Law. The formula and conditions for this Law are: pv=nrt and STP. n stands for the number of moles of gas, p is pressure, v is volume, r is a constant, and t is temperature. STP stands for standard temperature and pressure, which is 0 atm and 273 Kelvin. These conditions are when gases are "ideal." Obviously, gases do not always exist in these conditions, and therefore we can discuss trends associated with this equation.
I have attached a worksheet that we will complete in class to explain what each mean and which relationship they represent. The most important thing to remember in that the Ideal Gas Law takes into account the amount of Moles of a gas that is present and can only be used for ideal gases, which has several limitations that we will talk about in class.
I have also attached a link that has a general definition of what each law's relationship is. Please feel free to look around this website and familiarize yourself with the concepts and examples (Hint: a question on your next test may include a concept from this website). http://legacyweb.chemistry.ohio-state.edu/betha/nealGasLaw/
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