• 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

    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.

  2. IB chemistry revision notes

    o Soluble in polar solvents; insoluble in non polar solvents. * Usually requires differences of electronegativities larger than ~2. STATES OF MATTER Solids * Fixed shape- particles vibrate always (more at high temperatures) * Fixed Volume * Particles packed close together- hard to compress * Strong forces between the particles

  1. Group 4

    Therefore, the force on the body is smaller and fewer injuries result. When an airbag restrains the body, the body exerts an equal and opposite force on the airbag. Unlike the immovable steering wheel, the airbag is deflated slowly. This deflation can occur because of the presence of vents in the bag.

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

    the syringe connected to the pressure gauge and the pressure recorded to +/- 0.5 kPa. 2. The volume was then very gently decreased by 1.0 cm3 to 19.0 cm3 and allowed to stand for a minute and the pressure recorded after gently tapping the mechanical gauge.

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

    and ?HY (Trial 2) was taken. * ?HY = -106.3kJ.mol-1 Therefore, the standard enthalpy of reaction of reaction 2: MgO (s) + 2HCl (aq.) ? MgCl2 (aq.) + H2O (l) ------------ ?HX = -106.3kJ.mol-1 Calculating ?HMgO Since the enthalpies of reaction for both reaction 1 and reaction 2 are known, Hess? law can be applied and

  2. Chemistry lab reort-molar volume of hydrogen

    Hydrogen is weakly soluble in the water and these hydrogen bubbles might be dissolved in HCl solution instead of coming to the surface. This caused the measured value of hydrogen gas produced and thus the result of calculation to be slightly smaller than the actual values.

  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.

    when it accumulates in wetlands and there is poor drainage, could result in aquatic organism death. Its corrosiveness also adds to this. For HCFCs and HFCs to be effective alternatives to CFCs, they need to demonstrate first and foremost that they cause no (or minimal)

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