What is the internal energy of a gas whose volume is V?

Shooting star said: In an ideal gas whose volume is V, the internal energy is (3/2)PV. Actually, this can be re-written as 3/2 RT per mole (given that for a mole, PV = RT). So, indeed, for an ideal gas, only temperature matters for the internal energy.

How many kJ does a gas have?

As such, since neither the number of particles nor the temperature of the gas changes during the compression, the total internal energy of the gas also does not change. So, using c V = 20.8 J/ (mol K), n = 67 mol (the amount of air in 1500 L, and T = 300 K, we have that U = 418 kJ. The energy density

How do you find the internal energy of a molecule?

The program uses various equations of state to calculate the various data that it is capable of outputting. One equation of state for finding the internal energy is the Ideal Gas Law, which Shooting star has quoted you already. The 3/2 is however for the average translational kinetic energy of any kind of molecule in an ideal gas.

What is the energy of a gas under pressure?

The energy of a (perfect) gas under pressure is a tricky thing! In fact, a perfect gas is such that its energy is only dependent on its temperature U (T) and not on the pressure. But of course, a vessel under pressure can deliver work. So where's the issue ? It depends on how you expand the gas.

Does anyone know if a cylinder of compressed gas contains more energy?

Does anyone know if the energy in a cylinder of compressed gas/s (air) contains more energy or less energy than was used to compress it. doe is depend on nature of gas being compressed. A cylinder of compressed O2 by itself clearly would have a higher energy content than the energy consumer in compressing it, right.

How do you calculate internal energy?

Using the internal energy calculation U = 5/2PV I get 0.375MJ which is 0.00025MJ/L . (5L volume at 300 bar = 1500L total air. If I compress 1500L of air at 300 bar it can compress to 5L with total internal energy of 0.375MJ)