# Alka-Seltzer Co: Two Gases

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The main objective of this lab was to collect 〖Co〗_2 gases that were given off by the Alka-Seltzer tablets and to identify experimental masses. The volume of gas was 724 liters, or 723.86 cm and the experimental mass was .0894 grams. A balance scale was used before and after the reaction to record the change in overall mass. First, using the scale, the flask, balloon, and Alka-Setlzer tablets were measured, 259.4 ±.05 Grams were found. What created the “〖Co〗_2 gases to be trapped” were the crushed Alka-Seltzer tablets that went into the flask that contained water. The balloon that was attached to the flask was able to contain the 〖Co〗_2 that’s pressure was pushing forward, which helps one infer the rate of the chemical reaction. Throughout …show more content…
The 35 centimeters, the “border”, played a huge part in finding the volume of gas produced. By diving the 35 cm by 2 π, the radius was found. The radius, 5.57 cm, was plugged into the equation (4⁄(3 ) π)(〖5.57)〗^3 to give the answer 723.86 〖cm〗^3. Whats also important to point out is this needs to be converted into liters, and then it’s 724 liters. The ideal gas law, PV=nRT, was a formula that determined the number of moles produced. Taking the Barometric pressure, 769.9mmHg, and subtracting it from the volume of water, 17.5 mmHg, can formulate the pressure. Since pressure is what’s needed, 752.4 had to be divided by 760 to be converted into atm creating 0.99atm. Then with plugging in the rest, using .0821 and (20+273), the number of moles can be found by getting n, moles, alone. The answer then is .0298 moles of gas produced. After the reaction, and an incision to release the gas, the mass also had to be identified, which was less than the previous mass, 255.9 grams. The experimental molar mass was 0.0894 grams, found by using the moles of 〖Co〗_2 and the masses. The percent yield came about by dividing the experimental molar mass by the theoretical (44.01grams) to create 20 percent. The percent yield shows how far off the experimental calculations were from the truth. Overall, by using the Alka-Seltzer, what could be concluded was that Alka-Seltzer reacts

• ## Copper Nitrate Lab Report

Zn(NO3)2 Solution: 0.1M was chosen as the starting concentration for the Zn(NO3)2 solution, the same starting concentration as the copper (II) nitrate solution. In order to calculate the mass required to make a 200〖cm〗^3of 0.1M solution of Zn(NO3)2, the number of moles of the compound required must first be calculated. To calculate the number of moles required, the following equation was used: C=n/V (1 mol)/(dm^3 )=n/0.20 n=0.02 mol n=m/Mr 0.02mol=m/(65.37+(2(14.01+(3*16.00)) g/mol) 0.02mol=m/(189.39 g/mol) 3.788g=m Procedure: Place a plastic weigh boat on the 3 decimal scales, and then tare the scale. Then using a spatula, measure out 3.788g ±0.001g of Zn(NO3)2. Add this into the 500〖cm〗^3beaker.…

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• ## Daphnia Experiment Reaction Paper

The glass jars were filled in the same manner as the jars in the acute experiment. As an example, a 100 mg/L replicate would contain 2 mL of the buffered gibberellic acid 5000 mg/L stock solution and 98 mL of moderately hard water. In a similar manner as the acute experiment, the pH and the conductivity were recorded before the daphnids were placed in the jars. The daphnids were placed in the jars, after the jars were spiked, and allowed to equilibrate. There were four replicates for every concentration with every replicate having three…

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• ## Analysis Of Acetone And Toluene

However, this temperature was lower than the boiling point of acetone, the most volatile solvent possibly present in the unknown solution, pointing to a source of error in the measurement of the temperature. This could have been due to an inaccurate thermometer or to an error in placing the thermometer too high. Because the boiling point was so low, the more volatile solvent was estimated to be acetone, which has a boiling point of 56.5°C. After fraction A was collected, the temperature of the stillpot was increased and should have produced a steady increase in a plot of the temperature versus total volume distilled while fraction B (a mixture of the two components) was collected, until a second plateau at the boiling point of the less volatile component. The temperature of the stillpot needed to be increased after collecting fraction A because the liquid left in the stillpot was then composed of a higher percentage of the less volatile component, with a correspondingly higher vapor pressure, meaning that it would boil at a higher temperature.…

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• ## 1what Is An Acid-Base Titration?

The average of volume of NaOH used in the calculations was calculated as the average of the two best values which increases accuracy. The final pH of the titration can be altered if excess indicator is a added. Experiment 2: To prepare the solution of KIO3, the mass that must be added in 250 mL of distilled water must be calculated as shown; 1 mol of KIO3 is contain in 214.00g 0.005 mol of KIO3 1.07g Since the potassium iodate is only 99% pure 99% 1.07g 100% 1.081g Hence, mass of KIO3 used= 1.081g Apart from KIO3 and KI, sulfuric acid is also present in the conical flask, in excess, to provide H+ ions to increase the rate of reaction. 2.3 Conclusion After having done both experiment in the laboratory, we can conclude that he titration method relying on visual detection of the end point for quite precise determination of the unknown…

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• ## Thin Layer Chromatography

Using the equations and the numbers on Table 1 found in the data section, the Rf value for the isolated biphenyl was 0.66, the weight was 0.107 g, and recovery percentage was 35.7%. The pH level of the aqueous solvent was then manipulated from a base (sodium benzoate) back into an acid (benzoic acid), by adding HCl. The Rf value for benzoic acid was 0.115, the weight was 0.092 g and the recovery percentage was 30.7%. Using the equation shown in the data section, the total recovery weight came out to be 0.199 and the total recovery percentage was calculated to be…

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• ## 2.2 Preparation Of Inoculum

Helium was used as another carrier gas with the flow rate of 40mlmin-1. The heat-treated sludge was mixed thoroughly using the vortex [G-560 Scientific Industries, USA] prior to COD test, carbohydrate test and protein assay. The COD in the sludge was measured using spectrophotometer at 620 nm according to the Zhu et al. . The carbohydrate concentration was estimated by the phenol sulphuric acid method, using glucose as a standard .…

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• ## Copper Cycle Lab

This double displacement reaction was also supported from the equation when copper and sodium switched places in the products. In the third step of the cycle, after setting the heat to 355°, small amounts of a dark solid began to form at the bottom of the beaker. The liquid gave off steam, began to bubble, and turned a blackish color after a few minutes. After the solution cooled down, a dark black/brown precipitate was seen settled at the bottom portion of the beaker. In the fourth step of the cycle, the liquid was decanted and 10 mL of distilled water was added.…

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• ## Ideal Gas Law Experiment

13) Repeat steps 1-12 for the second trial. All data must be recorded in the second data table. 14) Add the two molecular masses together and then divide by two to find the average molecular mass of the C4H10. Also calculate the percent error of the experiment by using the experimental molecular mass of the C4H10 and the actual molecular mass of C4H10 (58g/mol). Data: First Trial: Mass of lighter before 11.09 g Mass of lighter after 10.60 g Mass of gas (M1 – M2) 0.49 g Initial V of H2O 308.0 ml Final V of H2O 99.0 ml V of gas (V1 – V2) 209.0 ml T of room 20.9 ° C/ 293.9 K Barometric Pressure 765.0 torr / 1.01 atm Water Vapor Pressure at 21° C 18.7 mm Hg /0.025 atm P of gas (barometric pressure – water vapor pressure) 0.985 atm Molecular Mass of gas 57.40 g/mol Second Trial: Mass of lighter before 10.60 g Mass of lighter after 10.10 g Mass of gas (M1 – M2) 0.50 g Initial V of H2O 307.1 ml Final V of H2O 87.1 ml V of gas (V1 – V2) 220.0 ml T of room 20.9 ° C/ 293.9 K Barometric Pressure 765.0 torr / 1.01 atm Water Vapor Pressure at 21° C 18.7 mm Hg /0.025…

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• ## Synthesizing Acetylsalicylic Acid

With excess acetic anhydride and a concentrated acid, 0.510 g of salicylic acid should have yielded approximately 0.665 g of acetylsalicylic acid. Unfortunately, small quantities of the reagents and products adhered to the sides of the flask and filter paper during the experimental process. In the end, an actual yield of 0.524 g resulted from the experimental procedures. This quantity equated to a 78.8 % yield. The purity of both the salicylic acid used and the acetylsalicylic acid recovered appeared high according to their observed and theoretical melting points.…

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• ## Separation Of Xylene Essay

 The operating pressure is 0.3kg/cm2 and 4.3 kg/cm2 in the second column.  All isomers of xylene was recovered from the column and were collected. The results obtained were 97 mole% benzene, 96 mole% toluene and 98 mole% xylene. In this process separation of acetonitrile from waste solvent acetonitrile is carried out.  The impurity contains isopropyl acetate, hydrogen cyanide, acrolein, oxazole.…

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