Chemistry Investigation 14: ------------------------------------------------- To determine the enthalpy change of reaction for: ------------------------------------------------- Na2CO3(aq) + H2O(l) + CO2(g) → 2NaHCO3(aq) Given: S1— Anhydrous sodium carbonate (Na2CO3) S2— Anhydrous sodium hydrogen carbonate (NaHCO3) A1—Aqueous sulfuric acid (H2SO4)‚ 0.500mol dm-3 Apparatus | Uncertainty | Measuring cylinder | ± 0.5 ml | Electronic Balance | ± 0.001 g | Data logger | ±0.2 ℃ |
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CHAPTER I INTRODUCTION 1.1 HISTORY: Ethylene Glycol (1‚ 2 – ethanediol)‚ HOCH2CH2OH usually called glycol is the simplest Diol. Diethylene glycol and Triethylene glycol are Oligomers of Mono ethylene glycol. Ethylene glycol was first prepared by Wurtz in 1859; treatment of 1‚2 dibromoethane with silver acetate yielding ethylene glycol diacetate via saponification with potassium hydroxide and in
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Thermodynamics- Enthalpy of Reaction and Hess’s Law Objectives: 1. To calculate the heat of reaction of a given reaction using the concepts derived from Hess’s Law. Pre-lab Questions: 1. Define Heat of Reaction. The enthalpy change associated with the completion of a chemical reaction. 2. Define Specific Heat. The energy it takes to raise the temperature of 1 gram of a substance by one degree Celsius. 3. Calculate the heat of reaction assuming no heat is lost to the calorimeter. Use correct
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Study material CHEMISTRY CLASS: XII KENDRIYA VIDYALAYA SANGATHAN LUCKNOW R E G I O N 2009-2010 Study Material Class XII -Chemistry SHRI RANGLAL JAMUDA IAS‚COMMISSIONER CHIEF Patron KENDRIYA VIDYALAYA SANGTHAN NEW DEHLI SHRI M.S Chauhan Asst. Commissioner Patron Kendriya Vidyalaya Sangthan Lucknow Region SHRI S.S. Rawat Guidance Smt. A.N Siddiqui (Education officer) (Education officer) SHrI K.‚M. Bhatnagar (Education officer) Co-ordinator SHRI. T. Singh Principal K.V. No. 2
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of unpaired (n - 1) d electrons‚ the stronger is the interatomic bonding and large amount of energy is required to overcome the interatomic interaction. ∆ fus Hθ M(s) → M(1) θ ∆ vap H M(1) → M(vapour) ∆a Hθ M(s) → M(g) These enthalpies are related as fus H < Dvap H < a H DOWNLOADED FROM WWW.STUDIESTODAY.COM DOWNLOADED FROM WWW.STUDIESTODAY.COM 76 XII – Chemistry AK DOWNLOADED FROM WWW.STUDIESTODAY.COM DOWNLOADED FROM WWW.STUDIESTODAY.COM The following
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surrounding the system * It takes energy to be organized lol * A cell is like an island of organization and it’s constantly fighting the sea of disorder to be organized. * Cells use energy from bonds of biomolecules (energy in bond is enthalpy) * Trade off is heat Table of approximate chem. Composition of e-coli shows that vast majority of energy goes into making macromolecules. * You can make polysaccharides from sugars * Fats/lipids/membrane from fatty acids * Proteins
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Ice Calorimeter Determination with Mg June 18th 2013 Abstract: This experiment determines the amount of energy needed to melt ice. A spontaneous increase in enthalpy produce by combining 0.2036g Mg and 5.00mL H₂SO₄‚ ice was melted and readings were taken by using an ice calorimeter. Readings were taken before during and after the reaction were completed. The data taken shows a value of -405 KJ/mol while the theoretical value was -483.7 KJ/mol. Calculating the experimental
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under kerosene oil because they get tarnished on exposure to air. 2. The general electron configuration of alkali metals is ns1. 3. Alkali metals have largest size and lowest ionization enthalpy in their respective periods. Down the group‚ the size of alkali metals increases whereas ionization enthalpy decreases. 4. Alkali metals have low densities and densities increases from Li to Cs. (Exception: K is lighter than Na‚ due to bigger size of potassium atom). 5. Alkali metals have low
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Honors Chemistry Chapter Nine PracticeExam Student: ___________________________________________________________________________ 1. Which of these compounds is most likely to be ionic? A. KF B. CCl4 C. CS2 D. CO2 E. ICl 2. Which of these compounds is most likely to be ionic? A. NCl3 B. BaCl2 C. CO D. SO2 E. SF4 3. Which of these compounds is most likely to be covalent? A. Rb2S B. SrCl2 C. CS2 D. CaO E. MgI2 4. Which of these compounds is most likely to be covalent?
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