Relation between temprature and pressure of a gas bieng compressed

In summary, the relationship between temperature and pressure of a gas being compressed is described by the Ideal Gas Law, which states that the product of pressure and volume is directly proportional to the product of the number of moles of gas and the temperature in Kelvin. Increasing the temperature of a gas while compressing it will cause the pressure to increase, as the average kinetic energy of the gas molecules increases. On the other hand, compressing a gas at a constant temperature will decrease its volume and increase its pressure, as described by Boyle's Law. Changing the number of gas molecules in a system while compressing it will also directly affect the pressure, with an increase in molecules leading to an increase in pressure. Finally, according to Charles's Law, at
1. If a gas is kept at constant pressure of 1 atm & the temp. is raised upto the saturation temprature ( 99.97 C ) and just when Tsat is attained the heat transfer is stopped ( Hin & Hout both are 0 , adiabatic conditions ) . Now
# If the adiabatic condition is maintained , then on increasing or decreasing the pressure the temprature will increase or decrease acc . how much will temprature change. will temprature reach to the new Tsat corresponding to the new pressure Psat?q

I have no idea what you are asking. Can you please restate this description more completely and precisely?

1. What is the relationship between temperature and pressure of a gas being compressed?

The relationship between temperature and pressure of a gas being compressed is known as the ideal gas law. It states that as the temperature of a gas increases, its pressure also increases, assuming the volume and amount of gas remain constant.

2. How does compressing a gas affect its temperature?

When a gas is compressed, its molecules are forced closer together, resulting in an increase in temperature. This is because the molecules have less space to move and collide with each other, causing them to gain kinetic energy and increase in temperature.

3. Does the type of gas being compressed affect the relationship between temperature and pressure?

Yes, the type of gas being compressed can affect the relationship between temperature and pressure. Different gases have different molecular structures and properties, which can affect how they respond to changes in temperature and pressure.

4. How does the volume of the gas being compressed impact the relationship between temperature and pressure?

The volume of the gas being compressed is directly related to the pressure and temperature. As the volume decreases, the pressure and temperature of the gas increase, and vice versa. This is known as Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at a constant temperature.

5. Can the relationship between temperature and pressure of a gas being compressed be applied to all gases?

No, the ideal gas law and other gas laws are based on certain assumptions and may not accurately apply to all gases. For example, at high pressures or low temperatures, gases may deviate from the ideal gas behavior, and additional factors may need to be considered in the relationship between temperature and pressure.

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