Essay Determining the Ideal Gas Constant

Beran, J. A. Laboratory Manual for Principles of General Chemistry. 8th ed. Hoboken, NJ: John Wiley & Sons, Inc.; 2009

Procedure: Have you made any changes to the procedure? Please explain. If you made no changes, state so. (1 point)

The Stages of Deception used as a way of Persuasion and the thought of Hope

In this experiment, two reactions were run to determine the molar absorptivity and the equilibrium constant of FeSCN2+. The main principles used in this lab are equilibrium, LeChatlier’s Principle, Beer’s Law and Spectrocopy. The first reaction was run to completion using LeChatier’s Principle and the second reaction was run to equilibrium. A spectrophotometer was used to measure absorbances. Using a graph of absorbance versus concentration of FeSCN2+ was used to determine that the molar absorptivity constant was 3670. Beer’s Law was used to determine that the average equilibrium constant was 33.1793.

In order to evaluate these equations, the obtained values of thermodynamic properties are compared with commonly used equations of state such as Peng-Robinson cubic equation of state, stiffened gas equation, isothermal Tait’s law, taking IAPWS-95 EOS for water and thermodynamic tables for CO2 and propane as the reference cases. Demonstrating a maximum error of 5 percent in liquid volume prediction, the present equation of state for liquid has a substantial superiority over the stiffened gas equation for the liquid phase volume prediction and in contrast to the Tait’s law, it can be employed for other fluids quite

13. In this experiment, the pressure (P) was 1 atm, the temperature (T) was 295 K, the volume (V) was 0.150 L, and the number of moles (n)was 6.2 * 10^-3 moles.   The ideal gas law states that P*V = n*R*T.  Based on your experiment, what value do you get for R?

Procedure: Refer to: Department of Chemistry, The Ohio State University. "Development of an Equation." General Chemistry 1210 Laboratory Manual. Vol. 2013-2014. Plymouth: Hayden-McNeil. 32-35.

Results show that the commissure displays the highest levels of variation, with one standard deviation reaching 1.5 ‰ for δ13C and 3.5 ‰ in δ18O values (Figure 4). These high levels at the commissure are similarly found at the umbo with standard deviations of 1.5‰ δ13C and 1.1 ‰ in δ18O. Both records show a “sweet spot” of low variation between 20-60% shell length (Figure 4).

ABSTRACT Recently there has an increase in developing a new line of preserves that instantly inflates when a seal is ruptured and two chemicals are allowed to fuse together. Applicants need to formulate and test a formula that gives the volume of the life preserver that would produce the minimum weight of sodium bicarbonate. Also, that when mixed with an excess of 1.0M HCl, it would inflate the life preserver to the pressure of 1300 torr using the following equation, NaHCO3 + HCl CO2 + H2O + NaCl. The objective of this experiment was to find out what was the least amount of sodium bicarbonate needed to react with an excess of 1.0 M HCl to inflate the bag. We were able to determine that around 22 grams of sodium bicarbonate were needed to firmly inflate the bag without bursting.

Since the literature value of 2-proponal at 20.6C is 4.41 kPa and the experimental value was 1.55 kPa, the literature value of ethanol at 20.4C is 5.97 kPa and the experimental value was 1.85 kPa, and the literature value of methanol at 20.5C is 13.32 kPa and the experimental value was 4.82 kPa it was evident that there were errors and limitations in the experiment. One error in the experiment was that the Vernier Pressure Sensor Kit never settled on one final pressure, the hundredths and tenths place kept changing so a final value had to be decided by group members. This error tried to be minimized by letting the pressure sensor run for 120 seconds, but the values still varied. Another error was that there were sometimes air gaps between

The “Gas Properties” simulation was opened. 2. Under “Constant Parameter” the “Volume” button was clicked on. This ensured that the volume remained the same. 3.

Overall, during the lab there should not have been too much error. This lab given us the opportunity to revised the data if necessary before continue to the next step. When we were asked to construct a Beer’s Law Calibration Curve we created a curve

period. The results were compared against standard curve developed using a concentration gradient of Na2So4 with BaCl2 (De Zoysa et al., 2007).

We want to try and develop a material balance equation that tries to give an accurate estimate of the original gas in place in a coalbed methane reservoir considering the absorbed gases, free gases, rock compressibility and certain factors that have strong effect on the original gas in place.

The details of the CV system used in this work are described elsewhere [15,16]. The design of the downstream compartment allows varying the volume for gas accumulation from 77.6×10-6 m3 to 1009.7×10-6 m3; at the same time, the effects of resistance to gas accumulation reported in ref. [31-33] are minimized. The absolute pressure transducer (MKS model 627B11TBC1B) to monitor gas accumulation operates in a range of 0 to 1333 Pa (10 torr), with an accuracy of 0.0133 Pa (0.0001 torr) and a maximum error of 0.12% of the pressure reading. This level of precision is typical of the best precision from pressure transducers currently available on the market. Prior to each experiment, the system is evacuated using a rotary vacuum pump (Edwards model RV3) for at least 48 h, and just before the experiment, leak tests for both upstream and downstream sides of the membrane are performed. During the leak tests, the vacuum pump is disconnected from the system and gas accumulation (if any) in the downstream reservoir is monitored for a period of time (from 20 minutes to 1 hour depending on the duration of the experiment).