What volume will 12.0 grams fo neon gas occupy at 25 degress C. and a pressure of 0.520atm?

To determine the volume of neon gas, we can make use of the ideal gas law equation. The ideal gas law is stated as:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)

To solve for the volume, we need to convert the given values to the appropriate units.

First, let's convert the temperature from degrees Celsius to Kelvin. We can do this by adding 273.15 to the given temperature:
25 degrees Celsius + 273.15 = 298.15 Kelvin

Next, we need to determine the number of moles of neon gas. We can use the formula:

moles = mass (in grams) / molar mass (in g/mole)

The molar mass of neon (Ne) is 20.18 g/mole.

moles = 12.0 grams / 20.18 g/mol = 0.5935 moles

Now we have all the necessary values to find the volume. Rearranging the formula and plugging in the values:

V = (nRT) / P

V = (0.5935 moles * 0.0821 L·atm/mol·K * 298.15 K) / 0.520 atm

V ≈ 15.83 liters

Therefore, 12.0 grams of neon gas will occupy approximately 15.83 liters at 25 degrees Celsius and a pressure of 0.520 atm.