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CHY 103 Lecture Notes - Lecture 6: Calcium Carbide, Joule

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School
Ryerson University
Department
Chemistry
Course
CHY 103
Professor
Noel George

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Document Summary

We have seen that calorimetry can be used to determine the enthalpy of reaction. Example: the one-step combustion of carbon to form carbon monoxide can be represented by. C (s) + 2 o2 (g) co (g) Rh = -110. 5 kj mol-1 or by the two-step process, C (s) + o2 (g) co2 (g) Co2 (g) co (g) + 2 o2 (g) The advantage: we can calculate the rh for almost any process by combining a series of reactions of known rh. Example: calculate rh for the reaction given the following information: No (g) + o (g) no2 (g) (1) (2) o3 (g) 3/2 o2 (g) (3) o2 (g) 2 o (g) No (g) + o3 (g) no2 (g) + o2 (g) Since enthalpies depend on conditions such as temperature and pressure a common set of conditions, the standard state was defined in order that enthalpies could be compared.

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Related Questions

1) What is the objective of this experiment? (Name of the experiment Introduction to Calorimetry)

A) To redefine Hess' Law.

B) To measure the light emitted from the reaction solution.

C) To measure the enthalpy of several acid-base reactions and to use these enthalpies along with Hess' law to determine the enthalpy of an acid base reaction not performed in the laboratory.

D)To study some of the properties of nable gases and thier reaction to acidic environments.

2) What is the SI unit for heat ?

A) Gallons.

B) Grams.

C) Moles.

D) Joules.

3) Which of the following has the units: J/gK?

A) Endothermic.
B) Specfic heat.
C) Enthalpy.
D) Heat capacity.

4) How would you define Specfic Heat (c)?

A) The amount of energy required to raise a mass one degree Celcius ( or Kelvin).

B) The change in temperature that occurs from one gram of substance releasing one Joule of energy.

C) The amount of heat required to raise one gram of a substance one degree Celcius (or Kelvin).

D) The amount of mass required to release one Joule of energy.

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.

The rate-determining step also involves the nucleophile. What is the nucleophile in the given SN2 reactions? Why does this nucleophile favor an SN2 reaction?