Find the Density of xenon of STP

D=PM/RT

Pressure= 1 atm
R= constant value (Use google)
T= 273K
For M.M of xenon use periodic table

To find the density of xenon at Standard Temperature and Pressure (STP), we need to know the molar mass of xenon and the values of STP.

STP refers to a temperature of 273.15 Kelvin (0 degrees Celsius) and a pressure of 1 atmosphere (atm).

1. Start by finding the molar mass of xenon.

The atomic mass of xenon (Xe) is approximately 131.293 grams per mole (g/mol). This value can be found on the periodic table or by searching online.

2. Use the ideal gas law to calculate the density.

The ideal gas law equation is given as:
PV = nRT

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

At STP, the temperature (T) is 273.15 K and the pressure (P) is 1 atm.

Assuming we have 1 mole of Xenon gas, we can rearrange the ideal gas law equation to solve for density (D):
D = (molar mass) / (RT/V)

Substituting the given values:
D = (131.293 g/mol) / ((0.0821 L·atm/(mol·K)) × (273.15 K) / 22.4 L)

3. Calculate the density.

Simplifying the equation, we get:
D = (131.293 g/mol) / (22.414 L·atm/(mol·K))

Calculating this, the density of xenon at STP is approximately 5.894 g/L.

So, the density of xenon at STP is 5.894 grams per liter (g/L).