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Heats of reaction

Heats of reaction. NaOH(s)  NaOH(aq) H= -4 3 .5 kJ NaOH(s) + HCl(aq)  NaCl(aq) + H 2 O H= -97. 0 kJ NaOH(aq) + HCl(aq)  NaCl(aq) + H 2 O H= -5 0 .2 kJ. NaOH dissolves (goes from solid to aqueous) NaOH dissolves and there is a reaction (neutralization) between NaOH and HCl

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Heats of reaction

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  1. Heats of reaction NaOH(s)  NaOH(aq) H= -43.5 kJ NaOH(s) + HCl(aq)  NaCl(aq) + H2O H= -97.0 kJ NaOH(aq) + HCl(aq) NaCl(aq) + H2O H= -50.2 kJ • NaOH dissolves (goes from solid to aqueous) • NaOH dissolves and there is a reaction (neutralization) between NaOH and HCl • The reaction between NaOH and HCl

  2. Definition of Hess’s law:for any reaction that can be written in steps, H is equal to the sum of the Hs for the individual steps 6. NaOH(s) + HCl(aq) 7. NaOH(s)  NaOH(aq) H= -43.5 kJ NaOH(aq) + HCl(aq)  NaCl(aq) + H2O H= -50.2 kJ NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) NaOH(s) + HCl(aq)  NaCl(aq) + H2O H= -93.7 kJ

  3. 8. E.g. the NaOH(s) takes some time to dissolve allowing heat to escape and perhaps giving artificially low values for changes in temp. E.g. the calorimeter is not perfectly insulated, thus larger jumps in temperature would not show up as high as they should For more lessons, visit www.chalkbored.com

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