Question

Calculate the pressure exerted by 10.2g of NH3 in a 3.0 dm3 vessel at 25deg celcius. a. Using ideal gas equation. b. Using Vander waals equation where constant. a =4.17dm6 atm mol-1. b=0.0371 dm3 mol-1

Answer 1

Calculate the pressure exerted by 10.2g of NH3 in a 3.0 dm3 vessel at 25°C .

a. Using ideal gas equation

b. Using Van der Waals equation where a = 4.17 dm³ atm mol¯¹ and b = 0.0371 dm³mol¯¹

solution : a. using ideal gas equation

PV = nRT

here volume, v = 3 dm³ ,

no of moles , n = 10.2/17 = 0.6

temperature, T = 25°C = 298K

P = nRT/V

= 0.6 × 0.082 × 298/3

= 4.8872 atm

b. using Van der Waals equation

(P + an²/V²)(V - nb) = nRT

⇒(P + 4.17 × 0.6²/3²)(3 - 0.6 × 0.0371) = 0.6 × 0.082 × 298

⇒(P + 0.1668)(3 - 0.02226) = 14.6616

⇒(P + 0.1668)(2.97774) = 14.6616

⇒P + 0.1668 = 4.92373411

⇒P = 4.75693411 ≈ 4.76 atm

Answer 2

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