Helium Gas Lab

11. Use the equation: q = m(SH)ΔT to solve for the specific heat of the metal.

To use the ideal gas law, the atmospheric pressure was adjusted for due to the lower pressure in the buret when compared to the outer atmospheric pressure. This unequalization of pressures, although corrected, may still be slightly off, thus potentially causing later calculation error when using the ideal gas law to solve for the moles of CO2.

In order to use the Ideal Gas Law equation, the atmospheric pressure of the room must be recorded from the barometer which was 0.9826 atm. The actual and theoretical yields can be calculated using the Idea Gas Law equation and the percent yield can then be determined. Finally,

The purpose of this lab was to determine the effect of temperature on the volume of gas when the pressure is consistent and to verify Charles’ Law. The data from the experiment reveals that as temperature increases, so does volume. This also indicates that as temperature decreases, the volume decreases as well.

As a result, it is a common practice to measure the volume of a gas by collecting said gas at the top of a container filled with water, with its opening facing downward in another container of water. This process is called collection of gas over water. The volume calculated from this practice may be used — in conjunction with two other factors (Pressure, Moles, or Temperature) — to determine another characteristic of a gas. This is able to occur due to the principles of the Ideal Gas Law. The Ideal Gas Law, PV=nRT, is derived from Boyle's Law, Charles Law, Avogadro's Law, and Gay-Lussac's Law,.

6. Select the lab book and click on the data link for Ideal Gas 1. In the Data Viewer window, select all the data by clicking on the Select All button and copy the data using CTRL-C for Windows or CMD-C for Macintosh. Paste the data into a spreadsheet program and create a graph with volume on the x-axis and pressure on the

The volume of a sample of oxygen is 300.0 mL when the pressure is 1 atm and the temperature is 27.0ºC. At what temperature is the volume 1.00 L and the pressure 0.500 atm?

28) A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage. What is the pressure of the basketball outside where the temperature is -1.00°C? A) 2.08 atm B) 1.80 atm C) 1.74 atm D) 2.00 atm 29) The density of a gas is 1.43 g/L at STP. What is the gas? A) Cl2 B) O2 C) S 30) Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) In an experiment, 201 mL of wet H2 is collected over water at 27°C and a barometric pressure of 733 torr. The vapor pressure of water at 27°C is 26.74 torr. The partial pressure of hydrogen in this experiment is __________ atm. A) 1.00 B) 706 C) 0.929 D) 0.964 E)

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.

b. Now increase the CO2 available to the elodea. What were your bubbles per minute? ______ bpm

The Teltron Tel 2533 Critical potentials tube contained neon gas kept at fixed, low pressure. Within this tube were a collector ring and a diode electron gun. The filament was kept at a fixed current of 1.2A. Any current higher than this would have done serious damage to the filament. The diode electron gun was used to emit a beam of electrons from its cathode. This beam passed from the cathode through the neon gas present in the tube to the anode. The collector ring within the critical potentials tube was connected to a fixed power supply of 1.25V and a Levell TM8 pA-meter to record the collector current. The fixed power supply of 1.25V was so that the collector ring was made positive relative to the anode. A variable accelerating

The hydrochloric acid is put into a calorimeter and then the zinc is added after. The lid is closed after the zinc is added and a thermometer is inserted through the lid in order to check the temperature as the reaction takes place . The temperature is measured until the reaction has completed and the highest temperature is used as the final temperature. ∆T is then found by the equation ∆T=Tfinal-Tinitial. Then according using the equation ∆H=mc ∆T+PV. In this lab the pressure remains constant while the volume is changing. In order to calculate the volume the same reaction with the same amount of zinc and hydrochloric acid is used. However, instead of a calorimeter, an erhlenmeyer flask with a balloon put over the top is used. The hydrochloric acid is placed into a flask, the zinc is placed inside the balloon and then sealed over the flask. By dropping the zinc into the flask the reaction occurs. This allows the H₂ gas to be captured in the balloon. The circumference of the balloon is then found. The circumference can then be applied to the equation C=2πr and the radius is determined. Using the radius of the balloon, in the equation V=(4/3)πr³ the volume taken up by the hydrogen gas can be found. The pressure is the pressure of the air which is measured with a barometer. ∆H can be found by multiplying the mass of hydrochloric acid, the specific heat of HCl, and ∆T of the hydrochloric

___The helium in the tank must be more dense than the helium in the balloons. ______________________________________________________________________

To achieve this, the final value from each thermocouple was set to be equal to the warm water bath temperature (370C), and the initial reading was set equal to the ice water bath temperature. Thus, for each thermocouple an equation was obtained using the two points to convert voltage readings to temperature. An example of the calibration for one of the thermocouples is shown in Appendix II.

The test tube labeled number one was placed in ice water at 0° Celsius. The number two test tube was exposed to room temperature at 25° Celsius. The number three test tube was placed in boiling water at 100° Celsius. After three minutes, the bubble’s height of the three test tubes were measured