Why do you need to use a polytropic process? This is an equilibrium problem.dbag123 said:what about using the polytropic process to figure out the partial pressure of the dry air at 1 atm?, the increase would be 0.3375 bar and that is the right answer, initial temperature is 90C
You need to assume that the change in the volume of liquid water is negligible.dbag123 said:in a jar that has an airtight lid there is water. Temperature is raised to 120C, from 90C, where the pressure of water vapor is 0,7 bar and the air 1 atm and as a result the pressure of the water vapor is 1,99bar. Calculate the partial pressure of dry air and the total pressure.
One could account for the density of the liquid water. However, since liquid water is approximately 1000 times as dense as steam at 2.0 bars, one might expect such an accounting to affect the result only in the third significant digit. The inputs here look to be good to only two digits at best.Chestermiller said:You need to assume that the change in the volume of liquid water is negligible.
An ideal gas pressure problem is a type of physics or chemistry problem that involves calculating the pressure of an ideal gas in a given situation. This type of problem typically involves using the ideal gas law, which relates the pressure, volume, temperature, and number of moles of a gas.
The ideal gas law is a mathematical equation that describes the behavior of ideal gases. It is written as PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
To solve an ideal gas pressure problem, you will need to use the ideal gas law and rearrange it to solve for the pressure (P). First, make sure all units are in the correct form (pressure in Pa, volume in m^3, temperature in K). Then, plug in the known values and solve for the unknown value (pressure).
The units for pressure in ideal gas problems are typically in Pascals (Pa). However, this can vary depending on the units used for volume and temperature in the problem. It is important to make sure all units are consistent when solving ideal gas problems.
The main assumptions made in ideal gas pressure problems are that the gas behaves ideally (following the ideal gas law), and that there are no intermolecular forces between gas particles. Additionally, the gas is assumed to be in a closed system and at a constant temperature.