I9 EXPERIMENT Charles'Law
MATERIALS
AND EQUIPMENT
125 mL Erlenmeyer flask, one-hole rubber stopper, glass and rubber tubing, pneumatic trough, thermometer, screw clamp.
DISCUSSION
The quantitative relationship between the volume and the absolute temperature of a gas is summartzed in Charles'law. This law states: at constant pressure, the volume of a particular sample of gas is directly proportional to the absolute temperature. Charles' law may be expressed mathematically: V ". T (constant pressure) V = kT o, : T = k (constant pressure) (1) (2)
where V is volume, T is Kelvin temperature, and k is a proportionality constant. dependent on the number of moles and the pressure of the gas. If the volume of the same sample of gas is measured
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Add water as needed to maintain the water level in the beaker. Read and record the temperature of the boiling water. While the flask is still in the boiling water, seal it by clamping the rubber tubing tightly with a screw clamp. Remove the flask from the hot water and submerge it in a pan of cold water, keeping the top down at all times to avoid losing air. Remove the screw clamp, letting the cold water flow into the flask. Keep the flask totally submerged for about 6 minutes to allow the flask and contents to attain the temperature of the water. Read and record the temperature of the water in the pan.
Figure 19. 1 Rubber stopper assembly
Figure
19.2
Heating the flask (and air) in boiling water
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In order to equalize the pressure inside the flask with that of the atmosphere, bring the water level in the flask to the same level as the water in the pan by raising or lowering the flask (see Figure 19.3). With the water levels equal, pinch the rubber tubing to close the flask. Remove the flask from the water and set it down on the laboratory bench. Using a graduated cylinder carefully measure and record the volume of liquid in the flask. Repeat the entire experiment. Use the same flask and flame dry again; make sure that the rubber stopper assembly is thoroughly dried inside and outside. After the second trial fill the flask to the brim with water and insert the stopper assembly to the mark, letting the glass and rubber frll to the top and overflow. Measure
Add RO water to the 25 ml volumetric flask up to the mark. Put stopper on the flask and shake it properly.
1. Move the lid of the container up or down. Record the resulting volume and pressure
Think about the gas laws we are studying. Boyle’s law tells us that pressure and volume are inversely proportional. Charles’ law states that volume and temperature are directly proportional. We also know that pressure and temperature are directly proportional. Discuss at least one instance in your personal experience where you have seen one or more of these laws in action.
In the lab we filled the first beaker up with water. Then we took a pipet (filled with the liquid) and dropped water droplets onto the
7. Based on your data, what relationship exists between the pressure and the volume of a gas (assuming a constant temperature)?
Suppose that the pressure of 1.00 L of gas is 380. mm Hg when the temperature is 200. K. At what temperature is the volume 2.00 L and the pressure 0.750 atm?
Can I apply this somehow to volume? Well at standard temperature and pressure (STP) a mole of a gas will occupy 22.4 liters. So If we keep our units straight we should be able calculate a given volume of gas from moles. Check it out…… http://www.sciencegeek.net/Chemistry/Video/Unit4/GMV4.shtml
Submerge the graduated cylinder in the plastic tub so that it is completely filled with water. Hold the open end of the graduated cylinder and move it vertically upside-down where the open end of the graduated cylinder is still submerged in the plastic tub. Clamp the graduated cylinder the ring stand of the lab table to keep it in place. perforate a hole in the top of the rubber cork for the solution container. Cut a straw the length of about four inches. place the straw inside of the rubber cork hole. Set up your timer for two minutes.
Robert Boyle, a philosopher and theologian, studied the properties of gases in the 17th century. He noticed that gases behave similarly to springs; when compressed or expanded, they tend to ‘spring’ back to their original volume. He published his findings in 1662 in a monograph entitled The Spring of the Air and Its Effects. You will make observations similar to those of Robert Boyle and learn about the relationship between the pressure and volume of an ideal gas.
3. The volume of a fixed mass of a liquid sample increases as the temperature rises from 20 to
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In the fourth stage of this experiment, the density of a gas was determined. A 250ml flask was weighed with an empty rubber balloon and the mass was recorded.
Place the beaker on the hot plate, place the thermometer in the beaker and set the hot plate to 5oC.
Carefully measure 75 of 1.0 M NaOH in a 100-ml graduated cylinder and pour it into the calorimeter. Leaving the thermometer out, place the top on the calorimeter.