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

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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.

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