• 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...


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.


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.


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


    The first of the major flaws in my experiment is that I assume once the reaction stops producing effervescence; it means that the reaction has stopped. This could cause inaccurate results because the reaction could still continue but not produce any more effervescence.

  2. IB chemistry revision notes

    The better down, the better the reducing agent. Use of Standard Electrode Potentials * Electrode potentials are a measure of how strong oxidising or reducing an agent is. They predict whether a redox reaction is energetically favourable. The hydrogen half-cell was used as the base for all the S.E.P.s E?

  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

    Overall, the calculations showed that very little error (0.36% error) which made me a little skeptical about the results. Such a small error percentage was not expected. To point out a few mistakes, I did not measure the difference in height of the water level from the surface of the water-filled container.

  1. Chemistry lab reort-molar volume of hydrogen

    The percentage uncertainties of the mole of hydrogen are 2% and 3% respectively, which are exactly the same as percentage uncertainties of the final results.

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

    Rubber is preferred over plastic because plastic gloves tend to tear very easily and hence risk jeopardizing the protection of hands. 1 × forceps/tweezers To be used to hold the Magnesium strips after cutting them from the ribbon 1 × spoon To scoop out MgO powder.

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

    = 0.0025 moles ________________ Utc.edu. < http://www.utc.edu/Faculty/Tom-Rybolt/121and122lecture/molecalculations.pdf>. ________________ * Percentage Deviation Percentage Deviation = 2.3 Data Presentation ________________ * Volume vs. Average Pressure Graph 2.1 shows the Volume of trapped gas (Air) in dm3 plotted against the Average pressure exerted by it in KPa. ?m = * 1/V vs.

  2. The chemistry of atmospheric and water pollution.

    Water is an essential substance for humans and we depend on it for survival. Thus it is essential that we continuously monitor water quality in local waterways, dams and especially in our drinking water. Contaminants and pollutants may be present in the water thus immediate removal is required to prevent any adverse affects on the human body.

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