Charles Law Lab Report

A sample of gas at 6.0 atm and 5.0ºC increases in temperature to 35ºC. If the volume is unchanged, what is the new pressure?

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

29. When the thermometer reads 40°C, carry the beaker out of the heating apparatus with a beaker tong.

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

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.

1. Move the lid of the container up or down. Record the resulting volume and pressure

Place the beaker on the hot plate, place the thermometer in the beaker and set the hot plate to 5oC.

The pressure of a gas sample increases for a decrease in volume and decreases for an increase in volume.

3. The volume of a fixed mass of a liquid sample increases as the temperature rises from 20 to

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.

Add RO water to the 25 ml volumetric flask up to the mark. Put stopper on the flask and shake it properly.

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.

Add 2 drops of soap to the removed test tube, and place it in the test tube holder.

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.