• 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. IB chemistry revision notes

    Catalysts * Increases the rate at which equilibrium is reached. The point of equilibrium does not change. * They affect backward and forward reactions equally. * Changes the reaction pathway for the reactions in question.

  2. THE CATALYTIC DECOMPOSITION OF HYDROGEN PEROXIDE

    To make this clearer, it means that catalysts only help to overcome activation energy in order to conserve the rest of the energy for the reaction. The more energy there is left the faster the reaction will be. This would explain why adding more catalyst causes an increase in the rate of decomposition.

  1. Determination of the molar mass of Magnesium from the reaction of magnesium and ...

    When the hydrochloric acid reached the magnesium ribbon, the reaction began. Hydrogen gas was formed pushing water out of the eudiometer through the rubber stopper hole into the measuring cylinder. After the reaction stopped, it was left for 5 minutes so that the eudiometer reaches room temperature.

  2. Group 4

    Hence, less serious injuries will occur, this will also help to save the driver's and passenger's life. This is how a simple chemical equation avoids the deaths of millions. Physic's Experiment Investigating safety on cars Introduction As cars became increasingly powerful and fast, rate of incidents increased exponentially and, usually more violent.

  1. Gas laws, investigate quantitatively the relationship between the pressure and volume for nitrogen ...

    Also, to make sure the needle of the gauge did not stick, the gauge was gently tapped before a pressure reading was taken. Design for the collection of sufficient relevant data: 1. To begin with, the 20.0 cm3 syringe was filled with 20.0 cm3 of nitrogen gas, the stopcock closed,

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

    and ?HX (Trial 2) was taken. * ?HX = -253.5kJ.mol-1 Therefore, the standard enthalpy of reaction of reaction 1: Mg (s) + 2HCl (aq.) ? MgCl2 (aq.) + H2 (g) ------------ ?HX = -253.5kJ.mol-1 For Part Y, Trial 1 Graphical analysis similar to that used in Part X has been

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

    ________________ Utc.edu. < http://www.utc.edu/Faculty/Tom-Rybolt/121and122lecture/molecalculations.pdf>. ________________ * Average Pressure 1Volume(dm30.0005) 2Pressure (KPa0.1) 3Average Pressure T1 T2 T3 Tav 0.060 91.8 91.8 91.8 91.8 Example: * Average Pressure = KPa Buchanan, L., Fensom, J. Kemp, E., La Rondie, P., & Stevens, J. (2012).Mathematics Standard Level.

  2. The chemistry of atmospheric and water pollution.

    A milky white precipitate confirms chloride ions. Carbonate ions can be tested by adding HCl and if it forms bubbles of CO2 then carbonate ions are present. Sulfate ions can be tested by adding barium ions to produce white precipitate of barium sulfate. Nitrate and phosphate ions tested using colorimetry.

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