A 1-m^3 container holds 50 g of hydrogen. The temperature is 20°C. Determine the pressure

Solutions

Expert Solution

Since H₂ gas is real gas so we can not apply Ideal gas equation directly

for this we have to apply real gas equation which is nothing but a modified ideal gas equation

which is also called Vanderwalls equation

Real gas Equation (P+an²/V² )*(V -nb) =nRT ......(1)

Where a and b are vander walls constant

a = attraction of gas molucules a = 0.2476 L² atm/mol²

b = volume of gas molecules b =0.02661 L/mol

n= no of moles of H₂ T = Temp in Kelvin R = Univ. gas const. V_cont. = volume in lit.

= given wt / mol.wt = 273.15 + temp in °C = 0.821 L.atm/mol.K = 1000 lit

= 50/2 = 25 mole =273.15+20 = 293.15 K

now putting the value of parametrs in ...equan (1)

(P+an²/V² )*(V -nb) =nRT

(P+0.2476*25²/1000² )*(1000 -25*0.02661) = 25*0.821 * 293.15

(P+0.00015475)*(1000 -0.66525) = 6016.90

(P+0.00015475)*999.33475 = 6016.90

(P+0.00015475) = 6016.90 /999.33475

(P+0.00015475) = 6.02

P = 6.02 - 0.00015

P = 6.0198 atm

P = 6.0198 atm this is answer

queen_honey_blossom answered 1 year ago

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