A researcher suspects that the pressure gauge on a 43.8-L gas cylinder containin

Question

A researcher suspects that the pressure gauge on a 43.8-L gas cylinder containing nitric oxide is broken. An empty gas cylinder weighs 115 lb. The weight of the partially full cylinder is 123.8 lb. This cylinder is located in a relatively chilly service hallway at 287 K. Follow the steps below to use the compressibility charts to estimate the pressure of the gas and the reading that the pressure gague should have. How many moles of nitric oxide, NO, are in the cylinder?

How many moles of nitric oxide,NO, are in the cylinder?

What is Vr ideal for nitric oxide?

What is the reduced temperature of the gas?

What is the reduced pressure of the gas?

What is the pressure inside the gas cylinder (absolute pressure)?

What should the pressure gauge read?

Explanation / Answer

weight of gas = 123.8-115 = 8.8 lb = 3.96 g

Molar mass of nitric oxide = 30 g/mole

Thus, moles of oxide = mass/molar mass = 0.132

Applying Ideal Gas Equation, Vr = (n*R*T)/P = (0.132*0.0821*287)/1 = 3.11 litres

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