# Molar Volume Of Gas Lab Report

1741 Words 7 Pages
Molar Volume of a Gas Lab The purpose of the lab was to do an experiment to determine the molar volume of hydrogen gas at standard temperature and pressure, or STP. To start the experiment, a beaker was filled with water and then a cage was created with a copper wire. A piece of magnesium was cut and placed inside the cage in order to keep the reaction going until all of the magnesium reacted with the hydrochloric acid. The eudiometer tube was filled with 15 mL of hydrochloric acid and water and then plugged with a one-hole rubber stopper that held the cage in place, ensuring that the magnesium would react with the excess hydrochloric acid. After covering the hole in the rubber stopper with a finger, the eudiometer tube was immediately inverted …show more content…
Avogadro’s law states that equal volumes of gas, at the same pressure and temperature, have the same amount of molecules. This applies to the lab in that it allows for the verification of the molar volume of hydrogen at standard temperature and pressure once temperature, pressure, and volume are all accounted for. Dalton’s law of partial pressure is another theory that was explored in this lab. It states that the total pressure of a mixture of gases is the sum of the partial pressures of the individual gases. This law makes it possible for the partial pressure of the water vapor to be removed from the total pressure of the gases in the eudiometer tube to yield the partial pressure of hydrogen gas. Molar volume is the volume occupied by one mole of a gas, in this case, hydrogen gas. Molar volume relates to the lab as the entire purpose of this lab is to find the molar volume of hydrogen gas at STP. The ideal gas law describes a relationship between pressure (P), volume (V), the number of moles (n), temperature (T), and the universal gas constant (R) where PV = nRT. This ideal gas law is essential to the lab as it explains the relationships between the different measurements of a gas and reduces into the combined gas law. The combined gas law is a relation where the number of moles of gas is constant, thus leaving the variables of pressure, volume, and temperature. When comparing the same substance under different conditions, the combined gas law can be mathematically written as (P"1" V"1" )/T"1" = (P"2" V"2" )/T"2" . Since the conditions of the experiment were not at standard temperature and pressure, the combined gas law is required in order to calculate the corresponding volume of hydrogen gas at STP. Single displacement reactions were also

• ## Lab Report: Moolar Volume Of A Gas At STP

Dalton’s Law was relevant in this experiment because it can be used to find the partial pressure exerted by the hydrogen by itself. It was hypothesized that if a gas is created through the reaction Mg + HCl → MgCl2 + H2 at a constant pressure and temperature, then the molar volume can be found out using gas laws because gases have direct and indirect relationships that can be used to find the unknown characteristic of said…

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• ## Enthalpy Lab Report

Temperature was measured during the reaction, allowing the amount of heat absorbed by the solution and the calorimeter to be measured. When added together, those values the enthalpy of the reaction. If the system loses no heat, this equation is true: “q_rxn=-q_soln-q_cal” (French et al, 105). This equation is equal to this one: “q_rxn=-m_soln s∆T-C_cal ∆T” (French et al, 105). For this reaction, s will be the specific heat of water because the experiment involves aqueous solutions.…

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• ## Molar Dehydration Experiment

Calorimetry allows for the heat of the solution to be calculated since the heat capacity of the calorimeter is known and the change in temperature is observed. The heat capacity is the ability for the container to retain the heat the is produced or absorbed without allowing for the outside environment to impact the reaction. This closed system allows for easy calculations where q_rxn+q_water+q_calorimeter=0. This is important to the lab that the total heat lost and gained must all equal zero. It would be hard to calculate how much heat was lost in the world by the experiment, so isolating the system to the calorimeter allows for the…

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• ## Limiting Reactants Lab Report

The graduated cylinder was then inverted, while the opening was still immersed in the water and it was attached to the ring stand using a clamp. It was set up so the opening of the cylinder was not touching the bottom of the basin, then the end of the tube was attached to the rubber stopper and inserted into the 500-mL graduated cylinder. The initial volume of gas within the cylinder was then recorded. A 250-mL Erlenmeyer flask was obtained. An amount of 0.100 grams of Magnesium was weighed and transferred to the flask.…

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• ## The Ideal Gas Law

Or simply, Ptotal = Pgas1 + Pgas2 + Pgas3 + Pgas4 + ... + Pgas n As previously mentioned, R is the ideal gas constant. In addition to being featured in the Ideal Gas Law equation, R is also used in other equations of thermodynamics. Officially R is equal to 8.314 (L∙kPa)/(mol∙K), 0.08206 (L∙atm)/(mol∙K), or 62.36 (L∙mmHg)/(mol∙K).  The objective of the lab is to prove the Ideal Gas Constant in the Ideal Gas Law. The gas, Butane, will be used to drain water from the Procedure A bucket was first filled with water and then the Graduated Cylinder to 250mL.…

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• ## Fuel Cells

Furthermore, in the straight pipe, a fully developed laminar assumption is satisfied under the condition that shape change is negligible. Numerical analysis technique the numerical analysis is performed by combining the governing equations related to the conservation of energy, conservation of mass and conservation of electrical charge to examine fluid distributions, heat transfers, mass transfers and electrochemical reactions. The assumptions used in developing the model are as follow: 1) Ideal gas law was employed for gaseous species. 2) The fluid flow in the fuel cell was laminar due to the low flow velocities and the small size of gas flow…

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• ## Heat Release Rate Model

The gross heat release rate is synthesized with an equation (3) having two separate Wiebe efficiency factors ap and ad in the two Wiebe functions often referred to as double Wiebe function [25, 33]. The direct experimental measurement of heat release rate is difficult. Therefore, a net apparent heat release rate calculated from the experimentally measured pressure-time profile and computationally calculated piston displacement profile along with heat loss to the cylinder wall using equation (1) is applied for validation. The diesel and DME oxidation reaction equations assuming complete…

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• ## Change In Enthalpy

Chemical reactions can be categorized based on the release or absorption of energy. For instance, chemical reactions that release energy are known as exothermic reactions and have a positive change in enthalpy. Moreover, chemical reactions that absorb energy are endothermic, which have a negative change in enthalpy. Since the energy released is usually heat, keeping track of the heat flow in reactions will help determine the change in enthalpy of a reaction. Observing the measurement of heat changes is known as calorimetry; hence, in this lab a calorimeter was used to measure the changes in enthalpy.…

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• ## Hydrogen Peroxide Decomposition Lab Report

Set time to 300 seconds. Step 4: Immediately cap the graduated cylinder with the gas pressure sensor to record initial rate Step 5: After the initial rate has been calculated, add 10 micro-liters of catalyst using a micropipette into the hydrogen peroxide Step 6: Measure the pressure build up of the catalyst with the hydrogen peroxide, again using the gas pressure sensor Step 7: Constantly stir the hydrogen peroxide with the magnetic stirrer to release oxygen gas trapped inside the solution Step 8: Add 10, 20, 30, and 40 ml of distilled water into the test tubes Step 9: Draw 1 mL of solution from the graduated cylinder with a micropipette and transfer it to test tube B and mix thoroughly. (The solution that originally had a volume of 10 ml now has a volume of 1 mL in test tube B. The solution, therefore, has been diluted by a factor of 10.) Step 10: Move 1 mL of the solution from test tube B to test tube C using the technique described previously and thoroughly mix the contents of test tube C. (The solution in test tube C has been diluted by a factor of 100.)…

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• ## Distillation Lab Report

Once at the stillhead, the pure vapor meets a water-cooled condenser that cools the vapor causing it to condensate and flow into a Falcon tube receiver. The Falcon tubes are utilized due to their graduated nature which make determining the volume collected easy. While watching the volume collected in the tubes, it is important to note the temperature at the stillhead because this is equivalent to the boiling point of the compound collected. A thermometer is placed here so that the tip of the mercury head is positioned with the bottom of the condenser. The thermometer will accumulate condensation and will accurately measure the boiling point of the collected compound.…

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