How many moles of helium are present in a 3.00L vessel at 435 mmHg pressure and at a temperature of 25 degrees Celcius? *
Answers
Explanation:
How many moles of helium are present in a 3.00L vessel at 435 mmHg pressure and at a temperature of 25 degrees Celcius? *
Concept:
Ideal Gas Equation.
PV = nRT
where P = Pressure of the gas
V = Volume of the gas
n = Number of moles of the gas
R = Gas Constant = 0.08206 L atm mol⁻¹K⁻¹
T = Temperature in kelvin
Given:
Pressure of the helium, P = 435 mm Hg = 435/760 atm
[to convert mm Hg to atm , we divide it by 760]
P = 0.5724 atm
Volume of the helium, V = 3.00 L
Temperature of the helium, T = 25°C = (25 + 273) K = 298 K
Find:
The number of moles of helium.
Solution:
As we know,
PV = nRT
n = PV/RT
Putting values in the above formula, we have
n = (0.5724)(3)/(0.08206)(298)
n = (1.7172)/24.45388
n = 0.0702 moles
Hence, the number of moles of helium is 0.0702.
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