• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Molar volume of hydrogen

Extracts from this document...

Introduction

Aim: To determine the volume of Hydrogen gas is produced when Magnesium reacts with Hydrochloric acid. Materials: Coil of Copper Wire, Hydrochloric Acid (3mol), 1.0 cm & 1.5 cm pieces of Magnesium strip. Stand and Clamp, Barometer, Thermometer, Beaker (200ml), Gas measuring tube Method: As on the experiment sheet Data Collection: Table 1.1 - The Length of the Magnesium strips with corresponding volumes of Hydrogen gas produced. Mg Length ( cm ) + 0.1 cm Mass Mg ( g ) + 0.001 g Volume 1 ( cm3 ) + 0.1 cm3 Volume 2 ( cm3 ) + 0.1 cm3 Volume 3 ( cm3 ) + 0.1 cm3 Average Volume ( cm3 ) + 0.3 cm3 1.0 0.021 17.2 18.0 17.8 17.7 1.5 0.032 27.0 26.8 28.3 27.4 2.0 0.043 36.0 36.0 37.0 36.3 2.5 0.053 49.0 43.5 46.3 3.0 0.064 56.0 53.8 54.9 3.5 0.076 58.4 58.4 4.0 0.085 67.8 67.8 4.5 0.094 77.0 81.2 79.1 Table 1.2 - Moles of hydrogen and the volume of hydrogen produced Moles of Hydrogen (mol) ...read more.

Middle

Measuring the amount of Hydrochloric Acid Measuring and cutting of Magnesium strips. Magnesium strips broken into pieces. Not taking the measurement of the volume of Hydrogen gas correctly due to parallax error. Uncertainties within Experiment: Measuring Cylinder � 0.05mL Gas measuring tube � 0.1mL Thermometer � 0.05�C Barometer � 0.05Kpa Ruler � 0.1mm 1. Calculate the mass and number of moles of magnesium used in your experiment. Number of moles used = mass of mg used (g) gram formula mass of mg (g/mol) = 0.021�0.1g 24.31 = 0.0008638 = 8.64 x 10 -4 � 0.1g 8.64 x 10 -4 � 0.1g moles of Magnesium was used. Calculate the number of moles of Hydrochloric acid. Moles of HCl = ( 8.64 x 10 -4) x 2 = 17.28 x 10 -4 = 1.73 x 10-3 � 0.2 2. From the partial pressure of water supplied calculate the partial pressure of Hydrogen using the formula. P atmosphere = P Hydrogen+ P water P atmosphere = 101.02 kPa � 0.1Kpa P Hydrogen =? ...read more.

Conclusion

Moles of hydrogen used against the volume of hydrogen produced. Moles of hydrogen against the volume of hydrogen produced, with a trend line and equation of the graph. 2. Describe the relationship between the two variables and indicate any proportionality that exists. The amount of Hydrogen gas that was produced is generally proportional to that of the moles used in the reaction. Although one point on the graph that is not proportional, this is most likely due to an error. Analysis Section: 3. From the graph determine the volume of hydrogen when the number of moles of hydrogen produced is 1.2 x 10-3 mol. Approximately 25.0cm3 of Hydrogen gas would be produced when the moles of hydrogen is 1.2 x 10-3. 4. From your graph calculate a constant of proportionality between the two variables (the gradient). Points: A (0.00129, 27.4) B (0.00172, 36.3) Gradient 1 = y2-y1 x2-x1 = 36.3 - 27.4 0.00172 - 0.00129 = 8.9 0.00043 = 20697.7cm3 = 20.7 dm3 Points: A (0.00344, 67.8) B (0.00387, 79.1) Gradient2 = y2-y1 x2-x1 = 79.1 - 67.8 0.00387 - 0.00344 = 11.3 0.00043 = 26279.07 cm3 = 26.3dm3 Average = 10.1 0.00043 = 23488.4 cm3 = 23.5 dm3 ?? ?? ?? ?? Chemistry Chemistry ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. THE CATALYTIC DECOMPOSITION OF HYDROGEN PEROXIDE

    Thus, this means that there would be large uncertainties in my data. To solve this problem, I should have used something else as my dependent variable, something else which is easier to determine. I could have set a fixed time for the reaction and measured the mass of content remaining

  2. IB chemistry revision notes

    * Rules for working out the structure: 1. Identify the central atom. 2. Work out how many electrons there are in the central atom.\ 3. Count the number of atoms bonded to the central atom ad then add that number to the number of valence electrons.

  1. Group 4

    However, the body does not continue moving at the same velocity for long, but rather comes to a stop when it hits some object in the car, such as the steering wheel or dashboard. Thus, there is a force exerted on the body to change its velocity.

  2. Chemitry Lab - Molar Volume of a Gas

    The error can come from - water vapour in the collection flask - 10cm water below the glass - air in the collection flask - temperature rise in the reaction flask - water vapour in the reaction flask Evaluation: This experiment had many error-causing factors, which probably influenced the results.

  1. Chemistry lab reort-molar volume of hydrogen

    Although the first result is less accurate, it has a higher precision than the second, more accurate one. The random uncertainty of the first is only , while the second has a relatively high random uncertainty of . The great difference between random uncertainties owes to difference in percentage errors of the mole of hydrogen gas produced.

  2. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

    1 × petri dish To be used when weighing out MgO powder. Petri dishes are easy to clean and the amount of powder on it can be adjusted very easily because they are shallow. 2 × rubber band To be used in making the Styrofoam cup calorimeter.

  1. Determining the relationship between the pressure and volume of a confined gas - Boyle's ...

    (2012).Mathematics Standard Level. New York: Oxford ________________ * R ? Ideal/Universal Gas Constant Boyle?s Law states that: Hence, nRT = 5.1589 91.8 = 16.67 * (0.0025 * 292.85 * R) R= 7.52 KPa.dm3.mol-1.Kelvin-1 ________________ *Temperature of syringe = 292.85 Kelvin ________________ *Number of moles of trapped gas (Air) = 0.0025 moles ________________ Utc.edu.

  2. The chemistry of atmospheric and water pollution.

    However besides these common ions, there may be other ions present ? e.g. NO3- and PO43- from fertilisers in the soil. The concentrations of the sodium and chloride ions need to be monitored as excess can increase salinity levels and aquatic organisms may not be able to cope with this.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work