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Chapter 5: Problem 112

Consider this apparatus. When a small amount of water is introduced into the flask by squeezing the bulb of the medicine dropper, water is squirted upward out of the long glass tubing. Explain this observation. (Hint: Hydrogen chloride gas is soluble in water.)

Short Answer

Expert verified
When water is squeezed into the flask containing Hydrogen Chloride gas, the gas dissolves in the water reducing the number of gas molecules and therefore the pressure inside the flask. The lower pressure inside as compared to outside causes the water to squirt out of the tube.

Step by step solution

01

Understanding of Hydrogen Chloride Solubility

Hydrogen chloride (HCl) is a gas that is highly soluble in water. When it comes into contact with water, it dissolves rapidly. This principle is outlined in Henry's Law, which states that at a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the pressure of that gas above the liquid.
02

Identifying the Pressure Change

When water is introduced into the flask, Hydrogen Chloride gets dissolved, reducing the amount of gaseous molecules in the flask. This decrease in the number of gas molecules causes a decrease in the pressure inside the flask, in accordance with Boyle's law which states that the pressure of a given amount of gas is inversely proportional to its volume, assuming the temperature remains constant.
03

Explaining the Water Squirt

The decreased pressure inside the flask creates a pressure difference between the inside and outside of the flask, with the pressure inside being lower than the pressure outside. This pressure difference causes the water to be forced upwards and squirt out from the long glass tubing. This principle is guided by Pascal's law that says a change in pressure at any point in a fluid is transmitted to all points in the fluid.

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Most popular questions from this chapter

At a certain temperature the speeds of six gaseous molecules in a container are \(2.0 \mathrm{~m} / \mathrm{s}, 2.2 \mathrm{~m} / \mathrm{s}, 2.6 \mathrm{~m} / \mathrm{s}\) \(2.7 \mathrm{~m} / \mathrm{s}, 3.3 \mathrm{~m} / \mathrm{s},\) and \(3.5 \mathrm{~m} / \mathrm{s} .\) Calculate the root- mean-square speed and the average speed of the molecules. These two average values are close to each other, but the root-mean-square value is always the larger of the two. Why?

A gas at \(772 \mathrm{mmHg}\) and \(35.0^{\circ} \mathrm{C}\) occupies a volume of \(6.85 \mathrm{~L}\). Calculate its volume at STP.

What are standard temperature and pressure (STP)? What is the significance of STP in relation to the volume of 1 mole of an ideal gas?

In 2012 , Felix Baumgartner jumped from a balloon roughly \(24 \mathrm{mi}\) above Earth, breaking the record for the highest skydive. He reached speeds of more than 700 miles per hour and became the first skydiver to exceed the speed of sound during free fall. The helium-filled plastic balloon used to carry Baumgartner to the edge of space was designed to expand to \(8.5 \times 10^{8} \mathrm{~L}\) in order to accommodate the low pressures at the altitude required to break the record. (a) Calculate the mass of helium in the balloon from the conditions at the time of the jump \((8.5 \times\) \(\left.10^{8} \mathrm{~L},-67.8^{\circ} \mathrm{C}, 0.027 \mathrm{mmHg}\right) .\) (b) Determine the volume of the helium in the balloon just before it was released, assuming a pressure of 1.0 atm and a temperature of \(23^{\circ} \mathrm{C}\).

What are the basic assumptions of the kinetic molecular theory of gases? How does the kinetic molecular theory explain Boyle's law, Charles' law, Avogadro's law, and Dalton's law of partial pressures?
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