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The Decomposition of Sodium Hydrogen Carbonate

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Introduction

TO FIND ?H FOR A REACTION WHICH IT IS NOT POSSIBLE TO MEASURE THE ENTHALPY CHANGE DIRECTLY ? In this experiment you are going to find ?Hreaction for the decomposition of sodium hydrogen carbonate: 2NaHCO3 (s) --> Na2CO3(s) + CO2(g) +H2O(l) by an indirect method. You are going to experimentally determine ?Hreaction for the reactions: Na2CO3(s) + 2HCl(aq)-->2NaCl(aq) + CO2(g) +H2O(l) and NaHCO3(s)+ 2HCl(aq)--> NaCl(aq) ...read more.

Middle

(i) To find ?Hreaction for Na2CO3(s) + 2HCl(aq)-->2NaCl(aq) + CO2(g) +H2O(l): ? Weigh out accurately about 2.0g of anhydrous sodium carbonate. ? Place 50cm� of the hydrochloric acid provided (in excess) in a plastic beaker. ? Record the temperature of the acid at half minute intervals. After 31/2 minutes add the anhydrous sodium carbonate, do not record the temperature. ? Stir vigorously with the thermometer. ? ...read more.

Conclusion

16.1 5 22.0 16.1 51/2 22.0 16.2 6 21.9 16.2 61/2 21.9 16.3 7 21.9 16.5 This table above shows the temperature change in �C. CALCULATIONS Sodium Carbonate Temperature Rise from 19.4�C to 22.0�C (a rise of 2.6�C)=2.6K Heat energy given out = mass of mixture x specific heat capacity x temperature rise of mixture M=0.05Kg Heat Capacity=4180J/Kg/K. Therefore heat given out= 0.05 x 4180 x 2.6 = 53.4 Kj. Using 2.07g of Na2CO3 (Mr=(23x2)+14+(16x3)=108) I.e. 2.07moles = 0.019167 108 ?H=53.4/1000 = 2.786KJ/mol or 2.79KJ/mol 0.019167 ...read more.

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