neutralization of 0.28M 18 mL sodium hydroxide with 0.5 mL nitric acid of 42% at the end of the reaction, a temperature increase of 15 °C was observed and the heat value was 825 cal it is determined. According to these results; a) The number of moles of the neutralized base is b) The enthalpy of reaction is c) The constant of the calorimeter in terms of water is (d(HNO3)= 1.51g/mL; M(HNO3)=63.01 g/mol) According to the enthalpy value, the reaction is

neutralization of 0.28M 18 mL sodium hydroxide with 0.5 mL nitric acid of 42% at the end of the reaction, a temperature increase of 15 °C was observed and the heat value was 825 cal it is determined. According to these results; a) The number of moles of the neutralized base is b) The enthalpy of reaction is c) The constant of the calorimeter in terms of water is (d(HNO3)= 1.51g/mL; M(HNO3)=63.01 g/mol) According to the enthalpy value, the reaction is

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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150 ml of .350M HCl was mixed with 150 mL of .350 M NaOH in a calorimeter of negligible heat capacity). The initial temperature of the HCL and NaOH solutions was the same, 23.25 degree C, and the final temperature of the mixed solution was 25.60 degrees C. Calcualte the heat of neutralization for the reaction: NaOH(aq) + HCl(aq) --> NaCl(aq) + H2O(l) dsol= 1.00 g/ml; S.H.sol = 4.184 J/g degree C
When 2.07 g of NaCl are added to 114 g of water in a constant pressure calorimeter, the temperature of the solution increases by 2.95 °C. Given that the molar mass of NaCl is 58.44 g/mol, and the specific heat of the solution is 4.184 J/g°C, what is the molar enthalpy of solution, AHsolution for NaCl in kJ/mol? Do not report units in your answer. Report your answer to one decimal place and include the correct sign.
Q) The heat of neutralization example: A 275 mL of a 0.500 M HClwas mixed with 275 mL of a 0.500 M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initialtemperature of the two solutions was room temperature(22.1 Celsius), and the final temperature of the mixed solutionwas 26.3 Celsius. Assume there is no heat lost to thesurroundings and the densities and specific heats of theinitial and final solutions are the same as for water (d = 1.00g/mL and s = 4.184 J/g.C). Calculate the molar heat ofneutralization for this reaction. Reference formula: constant Volume Calorimetry:~used for combustion reactions~done in the presence of XS oxygen gas~no heat or mass is transferred (isolated system)For the above calorimeter:qsys = qcal + qrxn = 0 b/c no heat is transferred! SOqrxn = -qcal where qcal = heat absorbed by the bombcalorimeter = CcalΔT
EXPERIMENTAL DATA ΔΗ -55.84 kJ/mol neutralization Mass of dry calorimeter, (g) 126.73 Initial burette reading, (mL) 0.31 Final burette reading, (mL) 14.31 Initial temperature of HCI, (°C) 22.30 Initial temperature of NaOH, (°C) 22.34 Mass of calorimeter and NaCl solution, (g) 156.89 Extrapolated temperature, T;, (°C) 38.26
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pl.s ans.wer
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Explain the following terms:(i) Internal energy of a system(ii) Bomb calorimeter
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