CHM 1311 Lecture Notes - Lecture 6: Eudiometer, Vapor Pressure, Former State Routes In Pennsylvania

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azuresardine419

23 Nov 2015

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In both trials a reaction occurred within few seconds once the mouth of the eudiometer containing the hcl and water was placed in the beaker and over the sample holder containing the magnesium. The reaction in this experiment produced a slight increase in heat causing the water in the beaker to heat up a few degrees above room temperature. In the first trial distilled water was used and several medium sized bubbles formed in this reaction. In the second trial tap water was used and more bubbles formed than in the first trial. As the bubbles formed in both trials the hcl and water in the eudiometer decreased quickly, forming hydrogen gas. The hydrogen gas also pushed down the water more rapidly than in the first trial. When the hydrogen gas was forming and water level decreasing the magnesium floated quickly up to the top of the water level in the eudiometer as it dissolved.

Related Questions

Show all the steps:

1) what will be the hydrogen pressure?

2) what will be the mass of Magnesium?

3) what will be the moles of hydrogen?

4) what will be percent by mass Mg?

can someone help me with this showing all steps? Thanks in advance.

Percent Magnesium in a Mixture Background In th is experiment you will determine the percent magnesium in a mixture containing only magne- sium and zine by reacting the sample with hydrochloric acid and measuring the volume of hydroger gas evolved. The reactions are: From the volume of hydrogen collected and its temperature and pressure, gen generated can be calculated. Using the stoichiometric relationships shown in the reactions above and knowing the total mass of zinc and magnesium, equations can be set up to solve for the individu al masses of the metals. the total moles of hydro- Determining the pressure of the hydrogen is a litle bit tricky. The hydrogen is collected over acid solution in a long calibrated tube called a gas measuring tube or eudiometer whi a beaker of water. The hydrogen pressure is not the barometric pressure. The total pressure in the eudiometer a ch is inverted in t the level of the liquid in the beaker is equal to the barometric pressure. This is the gas pressure plus the pressure due to the acid column above the liquid level in the beaker. To deter- mine the gas pressure barometric pressure. The column abo ure the pressure due to the acid column must be found and subtracted from the pressure of the acid column can be found by measuring the height of the ve the level of liquid in the beaker. Since we measure pressure as the height of a mercury column, the acid column height must be converted to mm Hg. The height of a liquid column sup- ported by a given pressure is inversely proportional to the density of the liquid. The density of the acid in the eudiometer is 1.05 e/mL and the density of mercury is 13.6 2/mL. Since the gas above the acid solution is hydrogen plus be subtracted from the gas pressure to get the pressure of the hydrogen alone. This is the pressure you will use in your calculations. Aqueous vapor pressures can be found in the table in Appendix C in your lab manual, or in the CRC Handbook which is available from the stockroom. water vapor and not pure hydrogen, the aqueous vapor pressure must pensi mercurs- 13.69/mL Volu me gas53. a melnic pressure 30 psi heiant of acal column 35.3 cm mass ââ corlonel metals= o.or68q

A sample of magnesium is reacted with of sulfuric acid as described in the experimental section. The resulting hydrogen gas is collected over water and is found to have a volume of . The temperature is and the atmospheric pressure is . The column of water inside the graduated cylinder is found to be .