Answer:
P₂ = 0.64 atm
Explanation:
Calculate the pressure exerted by 66.0 g of CO2 gas at -14.5°C that occupies a volume of 50.0 L
PV = nRT => P = nRT/V
P = ?
V = 50 Liters
n = 66g/44g·mol⁻¹ = 1.5mol
R = 0.08206L·atm/mol·K
T = -14.5°C = (-14.5 + 273)K = 258.5K
P = (1.5mol)(0.08206L·atm/mol·K)(258.5K)/(50L) =0.636atm=0.64atm (2 sig-fig)
The pressure exerted by 66.0 g of CO₂ gas at -14.5°C that occupies a volume of 50.0 L is 0.636 atm.
Pressure of any gas will be calculated by using the ideal gas equation as:
PV = nRT, where
P = pressure of gas = ?
V = volume of gas = 50L
R = universal gas constant = 0.082 L.atm/K.mol
T = temperature of gas = -14.5°C = 258.65 K
n is moles of gas and it will be calculated as:
n = W/M, where
W = given mass of CO₂ = 66g
M = molar mass of CO₂ = 44 g/mol
n = 66/44 = 1.5 moles
On putting values we get
P = (1.5)(0.082)(258.65) / (50)
P = 0.636 atm
Hence required pressure is 0.636 atm.
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