If 500 mol of hydrogen gas occupies 5.00L at 25 celsius, what is the pressure in atm?

I believe this is Ideal gas law. I can't figure out how to put it in the PV=nRT.

To solve this problem using the Ideal Gas Law equation PV = nRT, we need to rearrange the equation in order to solve for pressure (P). The equation becomes P = (nRT) / V.

Let's break down the given values:
- n is the number of moles of hydrogen gas, which is given as 500 mol.
- R is the ideal gas constant, which is a constant value equal to 0.0821 L.atm/(mol.K).
- T is the temperature in Kelvin. To convert Celsius to Kelvin, we need to add 273.15 to the given temperature of 25 °C, resulting in 25 + 273.15 = 298.15 K.
- V is the volume of the gas, which is given as 5.00 L.

Now we can substitute these values into the rearranged formula:
P = (nRT) / V
P = (500 mol) × (0.0821 L.atm/(mol.K)) × (298.15 K) / (5.00 L)

By performing the calculations, you will get the pressure in atmospheres (atm).

P = ?

V = 5.00 L
n = 500
R = 0.08205
T = 25+273 = 298
Substitute and solve.
I'm not sure I understand what your problem is.