The Physics Of The Gas

B. How does this graph illustrate Boyle’s law? As more pressure is added the volume decreases and the graph shows this because it is decreasing as well. _________________________________

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.

After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with the remaining NaOH until the colorless solution remained pink. The final volume was then recorded. While solution #1 was heating the same process was repeated with solution#2 and the second burette

8.When the reaction is completed, record the volume of gas in the graduated cylinder. Record observations about which reactant was the limiting reactant.

Carter heated up flask number three and did all the conditions to execute the experiment. Subsequently, Mr. Carter required a method of measuring how much gas was going to come out of the flasks. Due to the fact that he didn’t have a carbon dioxide meter or a gas pressure sensor, Mr. Carter used balloons to measure the fermentation process. The balloons will depict the results by showing us its growth from the carbon dioxide, from the fermentation process, filling it up. Although the balloons can’t quantify results, they provide visuals and will be accurate enough.

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.

These measurement was done by using a fixed amount of gas and a constant pressure and temperature. This way Boyle was able to examine the pressure-volume relationship without problems from other factors such as changes in temperature or amount of gas.

We put dry air, CO2, H2O (water vapor), and CH4 (Methane) each in separate, identical, empty water bottles. To create the dry air bottle, we just tightened a cap on an empty bottle. For the bottle with CO2, we used a combination of baking soda and vinegar. This combination produces a reaction that releases CO2. We simply poured the gas from this reaction into a bottle and tightened the cap. For the bottle with water vapor, we put a wet rolled paper towel into the bottle then tightened the cap. Professor Corbin prepared the methane (CH4) bottle with a gas jet. After creating the bottles, we measured the initial temperature of each bottle through small holes in the caps. Throughout the entire experiment, we were careful to keep the thermometer’s wire suspended in the middle of the bottle and not touching the side of the bottle. We also recorded the starting room temperature. We set up each bottle so that they were 9-12 inches away from the light bulb. We were careful to keep each bottle the same exact distance from the

The ideal gas law is expressed by the equation, PV=nRT. P refers to the pressure while V,n,R and T represent the volume, number of moles, the gas constant and the temperature, respectively. The ideal gas law describes the relationships between the properties mentioned above. Although this equation is widely used, it is limited in the sense that gases only behave “ideally” under very few circumstances. The moles of a substance are used here in addition to the volume.

Since Thanksgiving just passed I figured this was a good example! The temperature plunger on a turkey syringe thermometer pops out when the turkey is done. The gas law that is used in this example is Charles Law. “Charles’s law states that if a given quantity of gas is held at a constant pressure, its volume is directly proportional to the absolute temperature” ( Timberlake et al , 2007). This law basically means that temperature of the gas increases and gets higher , the gas molecules inside the turkey move around faster and hit the walls of the turkey which puts more and more force causing the volume to increase and the turkey syringe to pop out indicating that the turkey is done. The volume of air inside the turkey becomes trapped causing

To start with, a Netbook was set up by each group following the same steps. The temperature probe was connected to the LabPro and the netbook using an USB cord. The Labpro app was then started. File then New were selected to reset the app. The computer then needed to be prepared for data collection. To do this the file “Hess’s Law” was opened in the Chemistry with Vernier folder. A temperature probe was suspended using a clamp and a ring stand as demonstrated in the Principles to Chemistry 1 student manual on page 126 figure 9.1. A Styrofoam cup was placed in a beaker. 100.00mL of distilled water was measured out in a graduated cylinder, then poured into the cup. As Figure 9.1 shows, the probe was lowered into the the cup. To prevent contaminating, the

Neyra and I, under the influence of scientific curiosity, did the Boyle’s Law: Apparatus Lab to relate our results to the law. The lab places Boyle’s law into action to see if the lab results match up with the law. We hypothesized that the results of the experiment would correspond to the relation between volume and pressure established by Boyle. We began by setting up the cylinder apparatus by inserting the plunger into the cylinder and covering the plunger with a plunger platform. Once the apparatus was set, we began placing weights (pressure) and recording the volume in ml. To get a more accurate conclusion, we repeated the process four times. In fact, one trial consisted of adding consecutive number of weights (until four), and then removing them until there were zero weights left. Once we had our data recorded, we used the average of all trials to do calculations. After reading our data, we concluded that our hypothesize was very true to conclusions drawn by Boyle’s apparatus experiment. When there were more weights, the volume seemed to be smaller. However, once we started removing weights, the volume began to

At station 1 the balloon was heated causing the energetic particles to have lots of movement and bouncing resulting in the volume of the balloon to increase. At station 2 the balloon was chilled causing the energetic particles to not have much movement and bouncing resulting in the volume to decrease. At stations 1 and 2 the temperature did not change, but it still had an effect on the volume of the gas in the balloon…

This lab is to properly demonstrate how to find the Ideal Gas Constant, R, by using the ideal gas law, PV=nRt. In this equation, P is the gas pressure in the atmosphere, V is the gas volume (L), n is the number of moles in the gas, T is the gas temperature (K), and R is the gas constant. This ideal gas law helps determine the state of a gas at a certain amount, volume, temperature, and pressure. The hydrogen is collected by displacing water, which is submerging an object completely in water (gas buret) and recording how much the water rises. The volume of the water that is displaced can be measured and from this, the volume of the submerged object can be calculated. The hydrogen gas that is collected will also be mixed with water vapor, therefore

According to Boyle’s Law, the volume of any given amount of gas held at a constant temperature varies inversely with the applied pressure. In other words, when the pressure increases the volume decreases. When pressure decreases, volume increases. This can be derived from the following equation: