Answer:
74.08 atm
Explanation:
We'll begin by converting 91.7 kg to grams (g). This can be obtained as follow:
1 kg = 1000 g
Therefore,
91.7 kg = 91.7 kg × 1000 g / 1 kg
91.7 kg = 91700 g
Next, we shall determine the number of mole present in 91700 g of methane, CH₄. This can be obtained as follow:
Mass of CH₄ = 91700 g
Molar mass of CH₄ = 12 + (4"1)
= 12 + 4
= 16 g/mol
Mole of CH₄ =?
Mole = mass /Molar mass
Mole of CH₄ = 91700 / 16
Mole of CH₄ = 5731.25 moles
Next, we shall convert 497.9 gallon to litres (L). This can be obtained as follow:
1 gallon = 3.785 L
Therefore,
497.9 gallon = 497.9 × 3.785
497.9 gallon = 1884.55 L
Next, we shall convert 23.7 ˚C to Kelvin temperature. This can be obtained as follow:
T(K) = T(˚C) + 273
T(˚C) = 23.7 ˚C
T(K) = 23.7 °C + 273
T(K) = 296.7 K
Finally, we shall determine the pressure in the tank as follow:
Number of mole (n) = 5731.25
Volume = 1884.55 L
Temperature (T) = 296.7 K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure (P) =?
PV = nRT
P × 1884.55 = 5731.25 × 0.0821 × 296.7
P × 1884.55 = 139607.92
Divide both side by 1884.55
P = 139607.92 / 1884.55
P = 74.08 atm
Therefore the pressure in the tank is 74.08 atm
