560 mL of Xe will equal how many moles @ STP?

To calculate the number of moles of xenon (Xe) in 560 mL at STP (Standard Temperature and Pressure), we first need to know the molar volume of a gas at STP.

At STP, one mole of any ideal gas occupies a volume of 22.4 liters. Since we have the volume in milliliters, we need to convert it to liters by dividing by 1000.

Volume of Xe = 560 mL = 560/1000 = 0.56 L

Now, we can use the ideal gas law, which states that:

PV = nRT

Where:
P is the pressure (in atmospheres)
V is the volume (in liters)
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 pressure is 1 atmosphere and temperature is 273 K.

Plugging in the values:

(1 atm) (0.56 L) = n (0.0821 L·atm/mol·K) (273 K)

Simplifying the equation:

0.56 = n (0.0821) (273)

0.56 = n (22.414)

Solving for n:

n = 0.56 / 22.414

n ≈ 0.0249 moles

Therefore, 560 mL of xenon (Xe) at STP is approximately equal to 0.0249 moles.