Avogadro's Law Lab Report

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In this experiment, the molar volume of Hydrogen gas was measured by proving Avogadro’s Law. Avogadro’s law or principle was explained as: “Equal volumes of gases at the same temperature and pressure contain equal number of particles.” (Dingrando, Tallman, Hainen, Wistrom, Chemistry: Matter and Change)
Avogadro’s Law is related to the molar volume, which is the volume of one mole at standard temperature and pressure. Standard temperature and pressure (STP) were established as 0.00oC or 273K and 1 atm or 760mmHg. The molar volume of Hydrogen gas was recognized as 22.4L at STP. In this lab, the actual volume of Hydrogen gas was derived using the single-replacement reaction: Mg(s) + 2HCl(s) MgCl2(aq) + H2
The Hydrochloric acid …show more content…
To measure the amount of gas produced in this reaction, the number of Hydrogen gas moles was determined using stoichiometry. The pressure exerted by the H2 gas was derived using Dalton’s Law of Partial Pressures: PH =Patm-PH O. The partial pressure of the Hydrogen gas is the pressure of the water subtracted from the atmospheric pressure. The actual molar volume was measured by plugging all the values previously derived into the Combined Gas Law Equation: P1V1 = P2V2 .

This equation was used to determine the value of V1, where P1= pressure of the H2, T1= room temperature, P2= 760 mmHg (pressure at STP), V2= 22.4L (volume of H2 gas at STP), and T2=273K (temperature at STP). This was a proportion that compared the values of Hydrogen gas at STP to the experimental data. Proportions compare two things equal to each other, so the simplified result should have been 22.4 L too.
The Kinetic Molecular Theory explains the properties of gases that were used to determine the equations to find the molar volume. The behavior of Hydrogen gas can be explained with this simple model of the Kinetic Molecular
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