Answer:
P = 0.0009417 atm
Or,
P = 9.417 × 10⁻⁴ atm
Or,
P = 0.0954157 kPa
Or,
P = 0.715677 mmHg (Torr)
Explanation:
Data Given:
Moles = n = 3.2 mol
Temperature = T = 312 K
Pressure = P = ?
Volume = V = 87 m³ = 87000 L
Formula Used:
Let's assume that the gas is acting as an Ideal gas, the according to Ideal Gas Equation,
P V = n R T
where; R = Universal Gas Constant = 0.082057 atm.L.mol⁻¹.K⁻¹
Solving Equation for P,
P = n R T / V
Putting Values,
P = (3.2 mol × 0.082057 atm.L.mol⁻¹.K⁻¹ × 312 K) ÷ 87000 L
P = 0.0009417 atm
Or,
P = 9.417 × 10⁻⁴ atm
Or,
P = 0.0954157 kPa
Or,
P = 0.715677 mmHg (Torr)
Answer:
The correct answer is 95.36 Pa.
Explanation:
It is given that the moles of an ideal gas, n = 3.2 moles
Volume of an ideal gas, V = 87 m³
Temperature, T = 312 K
Pressure, P = x
The ideal gas equation, PV = nRT, here R is the gas constant, and at standard temperature and pressure, one mole of ideal gas holds 22.4 L volume, At STP, T = 0 degree C = 273 K
V = 22.4 L
moles, n = 1 mole
Gas constant, R = PV / nT
R = 1 atm × 22.4 L / 1 mole × 273 K
1 atm = 1.013 × 10⁵ Pa and 1L = 10⁻³ m³
R = 8.31 Pa. m³. mol⁻¹. K⁻¹
Now, there is a need to calculate pressure, P:
PV = nRT
P = 3.2 mol × 8.31 Pa. m³. mol⁻¹. K⁻¹ × 312 K / 87 m³
P = 8296.7 / 87
P = 95.36 Pa
