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

Enthalpy of Hydration Lab

Extracts from this document...


Marina Horta Enthalpy of Hydration Lab October 29/09 Abstract; The purpose of this experiment was to calculate the enthalpy of hydration for Magnesium Sulfate. Using the enthalpy of dissolution and Hess's Law the results of this lab were calculated to be -17197.18 kj mol-1. Using the graphs as a reference the final calculation can be determined to be on average correct. Introduction; The formation of a solution involves the interaction of solute with solvent molecules. When a solute is dissolved there are three energy process involved; The first is the separation of the solvent molecules which requires energy and so is an endothermic reaction, the second is also and endothermic reaction, the separation of the solute ions or molecules, and last is the attractive force between the solute molecules and the solvent, releasing energy ,exothermic. ...read more.


4 H2 (g) + 3C (s) +103.8 kJ 4 H2 (g) + 2 O2 (g) 4 H2O (g) -968 kJ 3 C (s) + 3 O2 (g) 3 CO2 (g) -1180.5 kJ which says that the enthalpy change is independent from the path taken and only the final and initial values matter. The values for each set will either result in a negative indicating an exothermic reaction or positive indicating an endothermic. The enthalpy of hydration can then be determined using the following equation; Materials; Styrofoam cups with lid, 50 ml volumetric pipette, stir plate and stir bar, ring stand and ring clamp, temperature probe, Xplorer GLX Data logger Distilled water, Anhydrous Magnesium Sulfate, Magnesium Sulfate hepathydrate Safety; MgSo4 is a hygroscopic and irritant MgSo4 * 7H2O is an irritant Calculations; Anhydrous trial 1 (3.49 g) ...read more.


The second two experimental graphs are negative for the anhydrous and show an exothermic reaction where the breaking of bonds between the solute and solvent releases energy and the graphs shows an increase in temperature with the addition of the solute. In comparison with other students however the results of this lab were too low, any error that can be attributed is most likely due to errors in calculations because the graphs used seem to be somewhat correct. Any experimental error that occurred would have been that not all of the solute dissolved, not allowing for the graph to be accurate. Leaving the anhydrous uncovered for any amount of time could also have added to error in calculations if any moisture was absorbed ( at this time humidity levels were higher) causing added weight. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Classifying Materials 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 GCSE Classifying Materials essays

  1. Iron Oxalate Lab

    absorbed light at different wavelengths in the electromagnetic spectrum in comparison it to the initial tests of blank and dark trails is used to measure the concentration of solutions using Beers Law. Beer's Law describes between the relationship between absorption of energy measured and its concentration, where A is absorbance,

  2. Rate of reaction of hydrochloric acid on magnesium.

    2.8cm3 but 0.4M the gas produced was 3.3cm3 at that same time. This is another factor that clarifies at higher concentrations hydrogen released is quicker therefore faster the rate of reaction. This table shows the rate of reaction for each concentration of HCl.


    Heat affects these particles, and increases there kinetic levels, allowing them to move faster. The same thing happens in water as so in this experiment, when the heat increases the kinetic energy of the water molecules there for allowing them to have a better chance of collision wit the dry spaghetti.

  2. Which equatoin is correct

    To produce one mole of gas by either of the equation the mass of one mole of CuCO3 can be calculated. This can be done using the formula M = m / Mr, where 'M' is the number of moles of substance; 'm' is the mass in grams; and 'Mr' is mass of 1 mole in grams ?

  1. Particulate Nature of Matter

    The six changes of state * Melting is the change from a solid to a liquid. * Vaporization is the change from a liquid to a gas.

  2. Specific Heat Lab

    to Error Q = (Error a/a + Error b/b...)*q. Because we used cmetal= (mh2o*ch2o*(Ti-Te)h2o)/(mmetal*(Ti-Te)metal) we need to add the estimated error of Te and Ti and use the formula above for the multiplications. cmetal= (mh2o*(Ti-Te)h2o)/(mmetal*(Ti-Te)metal) - We ignore the specific heat of H2O because no error is present. cmetal= (0 .005* 0.10)/( 0.005*0.10)

  1. Antimatter and matter

    Although Dirac may not have been the most sociable person, the consequences of his physics can certainly be mind-boggling. Here are ten Dirac facts that you might not have known... Ten Dirac facts 1. Antimatter is the most expensive stuff on earth at $62.5 trillion a gram.

  2. An experiment to investigate the factors that determine the amount of energy released when ...

    to supply the alcohol for complete combustion, and it would therefore produce the maximum amount of energy. Any further increase in the amount of oxygen will not have an effect on amount of energy produced. This is shown in the graph on the right.

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