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

Which Equation Is Correct for the following reaction with Copper Carbonate?

Extracts from this document...


Which Equation Is Correct? Copper has two oxides When Copper decomposes with heat two possible oxides are formed. Equation 1 2CuCO (s) Cu O(g) + O (g) Equation 2 CuCO (s) CuO(s) + CO (g) From the equations above we can see that in both reactions gas is evolved and by collecting the gas produced we can accurately say which reaction is taking place. To find which equation is correct we can use ideas about the mole and the volume one mole of gas occupies at standard conditions. In the test it is very important to ensure a fair test and to do this certain things must be kept the same. Temperature, of the collected gas should be kept at room temperature care should be exercised when heating the sample of carbonate that the apparatus containg the gas evolved is not also heated. It may also be a good idea to let the gas evolved cool down for short period of time after the experiment has occurred. This is because gas at a higher temperature expands and so occupies a larger area than equivalent cooler gas. Prediction In heating the Copper Carbonate we are providing energy to break the bonds in the carbonate sample as bond breaking is an endothermic process relative to the system. It follows the sample is at a higher energy state than before heating so then products will be at a high energy level. ...read more.


Hold the graduated cylinder perpendicular in the water and read the bottom of the meniscus to determine the amount of water displaced by the gas. Record the temperature of the water (which will also be the same temperature of the gas) and obtain the barometric reading. Safety Wear safety goggles and an apron in the lab at all times. Do not ingest chemicals. Use caution around open flames. Caution students to remove the gas delivery tube from under the water as soon as bubbling stops. (If not, as the gases cool, water may be sucked back into the tube causing it to break.) This is an accurate experiment but their tends to be heavy loss of gas evolved We can reduce this loss by using sealent betewn gas tube and rubber stopper Procedure for secound possible test Assemble the apparatus shown (except for the test tube) and add water to the levels shown in the liter bottle and the beaker using water, use glycerol (glycerine) as a lubricant when inserting the piece of 6 mm glass tubing in the stopper that fits into test tube A. Glycerol may be used for the other connections. Fill tube F connecting the liter bottle C with beaker D by blowing through the rubber tube B (blow GENTLY) with the pinch clamp OPEN. Raise and lower beaker D to expel any air bubbles from tube F. ...read more.


When the apparatus is cool to the touch (which will require several minutes) equalize the pressure then close the pinch clamp. Remove test tube A from the apparatus, insert it in its supporting beaker, and weigh the assembly. Set aside for later reheating. Remove the stopper from the liter bottle, insert a thermometer into the liter bottle, leave for a few minutes, and record the temperature (as the temperature of the gas). Look up the vapor pressure of water at this temperature in the Table below and RECORD IT IN YOUR REPORT FORM. Measure the volume of water in Beaker D by pouring it into a graduated cylinder. Read the volume to the nearest mL and record in your report form. Reheat the test tube for 5 minutes, cool and reweigh. Repeat this procedure until the weight lost between heatings is no greater than 0.05 g. Use the last weight obtained to calculate the weight of oxygen lost from the sample. Dispose of the residue in the test tube by WASHING IT DOWN THE SINK WITH LOTS OF WATER. DO NOT THROW IT IN THE WASTEPAPER BASKET OR THE SOLID WASTE CONTAINERS. VAPOR PRESSURE OF WATER temp. (oC) Vapor Pressure temp. (oC) Vapor Pressure torr torr 18 15.5 24 22.4 19 16.5 25 23.8 20 17.5 26 25.2 21 18.6 27 26.7 22 19.8 28 28.3 23 21.2 29 30.0 DIAGRAM OF THE ASSEMBLY TO BE USED IN THE EXPERIMENT Tube F MUST NOT touch the bottom of the liter bottle (leave 1/4 inch gap). ...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. Application of Hess's Law

    4.18 Joules x change in temperature in degrees Celsius Calculations for ?H1: Mass of NaHCO3 used = 9.43 grams, 9.41 grams and 9.44 grams Volume of HCl (2M) used = 50cm3 For ?H1 the temperature changes in order were 8?C, 10?C and 10.5?C Heat taken in when NaHCO3 reacts with HCl = 1.

  2. The aim of this experiment is to answer the following question: What is the ...

    This reaction goes to completion however the ion produced is not easily measured so this reaction is preferred. Another way to get the reaction to reach equilibrium faster would be to reflux the mixture. However I can not do this as when the mixture cools down the equilibrium would shift again making the heating pointless.

  1. Which equation is correct?

    Hence, the total volume of gas produced = 75.1 cm3 + 18.7 cm3 = 93.8 cm3 (3 s.f.) This will be the amount of gas produced in equation 1. How to recognize which equation is right It was worked out in a previous calculation that 0.386 g of CuCO3 should produce 75cm� of gas, if Equation 2 is correct.

  2. making copper

    . . . . . . . . . . . . . . . 600,000 Indonesia . . . . . . . . . . . . . . . . . . . . . 380,000 Australia . . . . . . . . .

  1. The aim of this experiment is to discover which of the following equations is ...

    It can also be more accurate as there are a variety of syringe sizes all with different markings. This makes it easier to find a suitable syringe for the collection of the gas. Calculations Equation 1 The relative molecular mass of 1 mole of Copper Carbonate (Mr)

  2. Experiment: To determine the correct equation for the decomposition

    The colour will change from green to black (copper oxide). * Wait 5-10 minutes before measuring the volume of carbon dioxide produced as this will allow it to cool down to room temperature * Repeat the experiment to obtain another set of results.

  1. To find out which equation is correct by heating CuCO3 and seeing which oxide ...

    So I shall use a solid lump of Copper Carbonate with as closer shape as possible to the other ones I shall be using. Pressure - I will not have the ability to keep the pressure constant all the time however I can perform all of the experiments within the

  2. Determine the Decomposition of Copper Carbonate

    using the Ideal Gas Equation, determine the theoretical volume of carbon dioxide expected. 5. Do a percentage error calculation for the volume of carbon dioxide gas. 6. using the combined gas law, determine the volume of carbon dioxide gas generated at STP. 7. Find the moles of copper (II)

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