Molar Volume Of Di-Hydrogen Lab Report

About 80 mL of HCl was obtained and mixed with phenolphthalein. Using a LabQuest unit and Gas Pressure Sensor kit, the HCl mixture was added to the flask with the magnesium ribbon and allowed to react. When reaction was complete, the change of temperature and gas was recorded. This procedure was repeated for different masses of magnesium ribbon (masses found on page 89 of the lab manual). After the completed procedure, moles of H₂ produced in each trial were calculated. (The actual procedure can be found on pages 87-89 of the lab manual)

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,.

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

In this lab, the molar mass of a volatile liquid is determined based on its physical properties in the vapor state. In order to calculate the molar mass, the mass, temperature, pressure, and volume is measured independently and then converted to the correct units. Sample C was obtained at the beginning of the experiment, which was later informed to be ethanol. Based on the calculations made, the molar mass of the volatile liquid was 95.9 g/mol. However, compared to the known value of 46.1 g of ethanol, the value measured had a 108% error. Unfortunately, this was a very big percent error and may have been caused by incorrectly measuring the volume of the gas. Using the ideal gas law, the molar mass of a volatile compound was calculated in order

Both experiments were able to determine the yield of hydrogen gas by testing the effect of limiting reactants, balanced equations, stoichiometry, mole ratios and molar masses. Balanced equations are equations that have a balanced number of moles of each element on both sides of the equation. Molar mass is the sum of the atomic masses of all elements combined in a chemical substance. Mole rations can be determined using the coefficients of the reactants and products in the balanced equation. Mole ratios can be used to relate moles of product formed from a certain number of moles of a reactant. Stoichiometry is the method of using the relationship between two or more substances in a chemical reaction. The limiting reactant of a chemical reaction is the reactant that is used up first in the reaction and limits how much of the product can be formed. In experiment 2-1, a company wanted to know if magnesium or aluminum would be practical to use as an alternative to zinc to produce a given volume of hydrogen gas. In experiment 2-2, the company wants to know how to optimize the production of hydrogen gas and whether hydrochloric or sulfuric acids are reasonable alternatives for gas production. The The reactions performed in experiment 2-1

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)

If the volume of the combustion container is 10.0 L, calculate the final pressure in the container when the temperature is changed to 110.° C. (Assume no oxygen remains unreacted and that all products are gaseous.)

In this today’s lab, Percent Yield of Hydrogen Gas from Magnesium and Hydrochloric Acid, the purpose is to study the stoichiometry of H2 produced from the reaction between magnesium (Mg) and hydrochloric acid (HCl). The chemical equation for this reaction is Mg +2HCl -> MgCl2 + H2. It was predicted that 0.0029 moles of hydrogen gas would be formed from 0.07g of magnesium metal and 10 mL of hydrochloric acid. The hypothesis was proven correct based on an actual yield of 0.00299 moles of hydrogen gas. We know this because after measuring the volume and pressure of our results, we used the Ideal Gas Law Equation to calculate the number of moles. We also calculated the percent yield by dividing the experimental number of moles of hydrogen gas

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?

In 1909 S.P.L. Sorensen published a paper in Biochem Z in which he discussed the effect of H1+ ions on the activity of enzymes. In the paper he invented the term pH to describe this effect and defined it as the -log[H1+ ]. In 1924 Sorensen realized that the pH of a solution is a function of the "activity" of the H1+ ion not the concentration and published a second paper on the subject. A better definition would be pH=-log[aH1+ ], where aH1+ denotes the activity of the H1+ ion. The activity of an ion is a function of many variables of which concentration is one. It is unfortunate that chemistry texts use a definition for pH that has been obsolete for over 50 years.

An experiment was conducted that examined the rate of a reaction between Hydrochloric Acid (HCl) and Magnesium shot (Mg). In this experiment, the Ideal Gas Law was used to experimentally determine the overall rate law for this reaction: PV=nRT where P is the pressure, V is the volume, n is the moles, R is the rate constant, and T is the temperature. The magnesium metal was predicted to react with the acid and turn all of the Hydrogen atoms into a gas that would then be collected which would make it possible to measure how fast the pressure is changing, since pressure is dependent on how much gas is

Hello mother, it’s me, Richard. I know it’s been a long time but I figured it’s about time to write back. I’ve been living in Jamestown for these past 13 years, with a stable job and great friends. I just wanted to start over ever since my wife, Betty died back in England. I lost everything after her death, hope, dignity, money, etc. I decided to come to Jamestown to begin a new life filled with opportunities and companions. I haven’t written sooner because I was afraid that the family would be disappointed in me, for just running away from my problems. The thing is, I didn’t run away, I just started afresh. Anyway, the colony is located in a swampy area with a river flowing by with gruesome, dirty water. The stream isn’t resourceful for farming so it’s pretty hard to grow food here. That’s what

The primary goals of this experiment concern expanding upon the concept of molar mass and its applications to the study of chemistry (Beran, 2014). To this end, the effect of an unknown solute on the freezing point of a solvent, cyclohexane, was measured and noted in order to determine a positive or negative relationship between the two variables (Beran, 2014). Additionally, the molar mass of the nonvolatile and nonelectrolyte solid solute was ascertained (Beran, 2014).

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