The diagram shows two flasks (A and B), each of which has a volume of 10.0 liter

Question

The diagram shows two flasks (A and B), each of which has a volume of 10.0 liters and is fitted with a pressure gauge. Flask A contains 0.300 moles of chlorine gas. Flask B contains 13.6 grams of ammonia gas. The temperature of both flasks is 20 degree C. (a) Evaluate the ratio: (number of gas molecules in flask A) (number of gas molecules in flask B) (b) Evaluate the ratio: (pressure in flask A) (pressure in flask B) (c) When the tap between the flasks is opened the two gases mix and react: 3 Cl_2 (g) + 8 NH_3 (g) rightarrow N_2 (g) + 6 NH_4 CI(s) Calculate the readings on the pressure gauges at 20 degree C when this reaction is complete.

Explanation / Answer

We have the ideal gas equation,

PV = nRT

V = Volume =10 L + 10 L = 20 L ,

T = Temperature = (273+20)K = 293K

n = number of moles = 0.300 + (13.6/17) = 0.3 + 0.8=1.1

R = 0.082 L atm /K mole

Hence, pressure = P = nRT / V

or, P = (1.1 × 0.082 × 293)/20 = 1.321 atm = 1.321 ×101.325 KPa

or, P = 133.85 KPa

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