3. Write balanced chemical equations for the neutralization reactions used in this experiment. Identify the limiting reagent for each reaction and explain answers. Why is the concentration of H3PO4 solution 0.67 M and that of HCl 2.00 M?
4. Calculate the theoretical standard of molar enthalpies for the neutralization reactions using the standard molar enthalpies of formation (write net ionic equations first, then search for standard enthalpies of formation in thermodynamic data tables.)
in this experiment, it is about the enthalpy of neutralization reactions between HCl and NaOH, and then replacing HCl with H3PO4 towards the end. we are first asked to determine the calorimeter constant, then the molar enthalpy of the NaOH and HCl neutralization, and lastly the molar enthalpy neutralization of H3PO4 and NaOH.
3. Write balanced chemical equations for the neutralization reactions used in this experiment. Identify the limiting reagent for each reaction and explain answers. Why is the concentration of H3PO4 solution 0.67 M and that of HCl 2.00 M?
4. Calculate the theoretical standard of molar enthalpies for the neutralization reactions using the standard molar enthalpies of formation (write net ionic equations first, then search for standard enthalpies of formation in thermodynamic data tables.)
in this experiment, it is about the enthalpy of neutralization reactions between HCl and NaOH, and then replacing HCl with H3PO4 towards the end. we are first asked to determine the calorimeter constant, then the molar enthalpy of the NaOH and HCl neutralization, and lastly the molar enthalpy neutralization of H3PO4 and NaOH.
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