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

Investigating the energy change in reactions involving metals

Extracts from this document...

Introduction

Investigating the energy change in reactions involving metals Aim To find the energy change as we react several group one elements with hydrochloric acid. Hypothesis1 The reactivity of a metal is directly proportional to its position on the periodic table of elements, and is determined by the number of protons and the number of electron shells the atom has. It is said that metals become stronger and more reactive as you move left, because there are less electrons which need to be lost. Metals are also more reactive as you move down the table because the atomic radius becomes larger to an extra filled electron shell, making the outer electrons further away from the nucleus. Electrons are held in their shells by a force from the protons in the nucleus, and the further away the outer electrons are from the nucleus, the less of a pull the nucleus will be able to exert in order to hold the outer electron. Because I have chosen to find the energy change in group one elements, I predict that all three metals, Lithium, Sodium and Potassium, will react violently with hydrochloric acid. More specifically, I hypothesize that Lithium, atomic number 3, will be the least reactive, and thus will produce the least amount of energy. ...read more.

Middle

+ 2HCl(aq) = H2(g) + 2NaCl(aq) Total ionic equation: 2Na(s) + 2H+1(aq) + 2Cl-1(aq) = H2(g) + 2Na+1(aq) + 2Cl-1(aq) Net ionic equation: 2Na(s) + 2H+1(aq) = H2(g) + 2Na+1(aq) Oxidation: 2Na(s) = 2Na+1(aq) + 2e- Reduction: 2H+1 + 2e- = H2(g) Potassium & Hydrochloric acid - Balanced equation: 2K(s) + 2HCl(aq) = H2(g) + 2KCl(aq) Total ionic equation: 2K(s) + 2H+1(aq) + 2Cl-1(aq) = H2(g) + 2K+1(aq) + 2Cl-1(aq) Net ionic equation: 2K(s) + 2H+1(aq) = H2(g) + 2K+1(aq) Oxidation: 2K(s) = 2K+1(aq) + 2e- Reduction: 2H+1 + 2e- = H2(g) For more accurate analysis, we should convert the amount of metal used from grams to moles. In order to do so, we must divide the weight, in grams, by the atomic mass: Lithium: 0.03 / 6.94 = 0.004 Sodium: 0.03 / 22.99 = 0.001 Potassium: 0.03 / 39.10 = 0.0007 Conclusion My aim was to find the change in energy by reacting lithium, sodium and potassium with hydrochloric acid. I was able to do this successfully by first measuring the temperature of the solution right before and after the reaction, then finding the change in temperature, and from there finding the energy produced for each metal. As you can see from the tables and graph above, we managed to gather fairly good results. ...read more.

Conclusion

Also, we could look at the smaller things, like the uncontrolled variables, which can sometimes have a very big effect on results, such as air pressure and room temperature. Another problem, as I have mentioned earlier, is how we used grams to measure the weight of the metals instead of moles. This directly interfered with our results as it gave us the complete opposite figures, which can also be seen as one of the factors which makes our results unreliable. This can also be used as an improvement or something to bear in mind in case I ever repeat a similar experiment, because if I use moles instead of grams, then I am able to truly test my hypothesis. Another improvement, or a way to take my experiment further, would be by using the same elements, but in different solvents; for example, in sulphuric and nitric acid, as well as water. Also, I could work with all the group one elements, using moles, so I could fully test the theory that metals become more reactive as we descend. Also, I could experiment across the periodic table of elements, or only test the transition metals in acid, to see what happens, and hopefully, find some successful patterns and comparisons. Furthermore, I could try measure the energy change with pH, to see if there was any difference. 1Scientific information from hypothesis obtained from : http://richardbowles.tripod.com/chemistry/reactivity/reactivity.htm ?? ?? ?? ?? 1 ...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 Aqueous 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 GCSE Aqueous Chemistry essays

  1. Reactivity of metals Investigation

    bit more vigorous and violent than the reaction between magnesium and HCL. The reactions are very similar because Magnesium is right behind Calcium in the reactivity series so the reactions are bound to be similar. * Magnesium + hydrochloric acid magnesium chloride + hydrogen + (heat) Mg(s) + 2HCL(aq) MgCL2(aq)

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    in 20 grams by 5. The spinach was boiled in Sulphuric Acid (aq) as this broke the spinach up completely and it formed a mush, and thus all the Iron (II) would be extracted from it. The solution was boiled to a temperature of 70 oc as this is hot

  1. To investigate the factors that affect the amount energy produced in neutralisation reactions.

    The procedure for this variable is also somewhat less complex than most of the others. The acids that I will use for my experiments will be one molar values of sulphuric, hydrochloric, nitric, Ethanoic, methanoic and citric acid. I will use one molar Sodium hydroxide for the course of the investigation.

  2. Determining the atomic mass of lithium from method one. After setting up my apparatus, ...

    + HCl(aq) _______Cl(aq) + H2O(l). The ratio of LiOH : HCL is 1 : 1 therefore the number of moles of LiOH = 0.002848moles The total volume of LiOH was 100cm3 Therefore 0.002848 � 4 = 0.011392 moles Going back to the first equation 2 Li(s) + 2 H2O(l)

  1. Investigating the kinetics involved in the reaction of metals with acids.

    Make sure the gas syring reads 0cm3 before starting the reaction. Reset the stop clock to zero and then pull the string from the conical flask to release the magnesium strip. As soon as the magnesium lands in the acid, start timing the reaction.

  2. Investigation into osmosis in plant tissue

    The graph is a negative strong correlation but there was an anomalous result, circled in green on the graph; it is 1.5mm longer than predicted. This is not too serious but a larger difference than all the others are from the line of best fit.

  1. Transition metals

    cutting tools * Transportation * Woks * Camp ovens * Household appliances Titanium Titanium is lightweight, strong and rust-resistant. Titanium is a silver-white metal. Pure titanium is quite soft but titanium alloys are extremely strong (even stronger than steel and aluminium).

  2. Alkali Metals.

    They also are utilized to remove impurities from copper and certain other metals. Lithium salts are added to glass, porcelain enamels, and ceramic glazes to render them heat-resistant. Some such salts, furthermore, are employed in experimental high-voltage batteries for electrically powered automobiles.

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