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CHM 1311 Study Guide - Limiting Reagent, Dgh, Room Temperature

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turquoisefox286

11 Jul 2014

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Experiment 1: determination of the composition of an alloy. Data and results in the determination of the composition of an alloy. Volume of hydrogen gas (ml) (a) volume of hydrogen gas after calibration (ml) Acceleration due to gravity (m/s2) (b) pressure of water column (kpa) Atmospheric pressure (c) pressure of hydrogen gas (kpa) Ideal gas constant, r (l kpa/mol k) (d) actual moles of hydrogen gas (mol) (e) theoretical moles of hydrogen gas (mol) (f) percent yield of h2 from magnesium (%) Data (g) volume of hydrogen gas after calibration (ml) (h) pressure of hydrogen gas (kpa) 94. 95 (i) actual moles of hydrogen gas (mol) 9. 400 10-4 (j) mass of aluminum (g) (k) mass of zinc (g) 3. 53 10-2 (l) percentage composition of alloy. *trial 2 values for magnesium test were cited, and the eudiometer tube used in cited work was already calibrated.

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Related Questions

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 .

1. What is the height of the water column after converting to an equivalent height of mercury in ?

2. What is the pressure of the hydrogen gas in the column in ?

3. What is the pressure in Question 2 in ?

4. What is the number of moles of hydrogen gas in the sample?

5. What is the number of moles of metal in the sample

6. What is the calculated molar mass of the metal for this trial?

7. What is the percent error in this determination?

goldjellyfish475

How do I get the correct pressure of hydrogen gas? Also is the question before this one correct?

I attached pics of my experimental results as well

Experiment 5: Calculations (NOT allowed on concept review, DO NOT pass in with report) You must be able to perform these calculations with given data on your concept review quz. Mass of Magneslum strig Calculate the mass of your magnesium strip by multiplying the mass of 1 meter of magnesium (grams) by the ength of your magnesium strip in centimeters and dividing by 100 to convert centimeters to meters. You may assume the magnesium ribbon was of uniform thickness and width. 34 9 Mass of magnesium strip00 Moles of magnesium used Calculate the moles of magnesium in the strip by dividing the mass of the magnesium strip by the molar mass of magnesium metal 0.600 2o males Mass Mp oOCs Moles of magnesium Molar Mass Ma 2.305 The number of moles of hydrogen gas produced, Ha, is equal to the moles of magnesium used up, since the mole ratio between the moles hydrogen gas and the moles of magnesium in the balanced equation for this 0.000 20g mous Moles of hydrogen gas By matching the level of water in the cylinder to that outside the cylinder, you can make the assumption that the gas in the cylinder is at atmospheric pressure. However, since you collected the gas over water, your atmospheric pressure is composed of the vapor pressure of the hydrogen and the vapor pressure of the water To accurately calculate R based on the hydrogen gas, you need to find the pressure exerted by the hydrogen gas only. Use Table 1 to find the vapor pressure of the water vapor in the graduated cylinder at roonm temperature in the lab and then subtract this from the atmospheric pressure given to you by your TA. Keep in mind that pressure can be measured several different ways. You will need to use these conversions to convert all pressures into atmospheres so the units will cancel when you use the ideal gas law to calculate R The most commonly used conversions are 1 atm 101.325 kPa = 760mm Hg 760 torr The equation for the partial pressure of hydrogen is: Prytrogen Pemophere-Pt Pressure of hydrogen gas 91