A thin glass tube 1 m long is filled with Ar gas at 101.3 kPa, and the ends are stoppered with cotton plugs as shown below. HCl gas is introduced at one end of the tube, and simultaneously NH3 gas is introduced at the other end. When the two gases diffuse through the cotton plugs down the tube and meet, a white ring appears due to the formation of NH4Cl1s2. At which location—a, b, or c—do you expect the ring to form?

Key Concepts

Graham's Law of Effusion

Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This means lighter gases will diffuse faster than heavier gases. In this scenario, NH3 (ammonia) has a lower molar mass than HCl (hydrochloric acid), which suggests that NH3 will travel further down the tube before the two gases meet.

Diffusion

Diffusion is the process by which gas molecules spread from areas of high concentration to areas of low concentration. In the context of the question, both HCl and NH3 gases will diffuse through the cotton plugs towards each other, and the rate at which they diffuse will determine where they meet and react to form NH4Cl.

Chemical Reaction and Product Formation

When HCl and NH3 gases meet, they react to form ammonium chloride (NH4Cl), which appears as a white ring. The location of this ring depends on the relative rates of diffusion of the two gases. Understanding the reaction and the conditions under which it occurs is crucial for predicting where the ring will form in the tube.