at what kelvin temperature will 25.2 of xe occupy a volume of 645 L at pressure of 732 torr?
No 25.2 is moles
To find the Kelvin temperature at which 25.2 moles of Xe (xenon) will occupy a volume of 645 L at a pressure of 732 torr, we can use the ideal gas law equation, which states:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L*atm/mol*K)
T = temperature (in Kelvin)
First, we need to convert the pressure from torr to atm by dividing it by 760 (since 1 atm = 760 torr), so:
P = 732 torr / 760 torr/atm ≈ 0.963 atm
Next, plug the values into the ideal gas law equation and solve for T:
0.963 atm * 645 L = 25.2 mol * 0.0821 L*atm/mol*K * T
Rearranging the equation to solve for T:
T = (0.963 atm * 645 L) / (25.2 mol * 0.0821 L*atm/mol)
T ≈ 255 K
Therefore, at approximately 255 Kelvin temperature, 25.2 moles of Xe will occupy a volume of 645 L at a pressure of 732 torr.