Accelerated ChemistryChapters 16 and 17 Worksheet #1Name ______

  1. Calculate the Heat of Reaction using Bond Energies:

H2+O2H2O(Don’t forget to balance!)

CH4C2H6+H2

C2H5OH+O2CO2+H2O

(over)

  1. Calculate the Heat of Reaction using Hess’ Law:Don’t forget to balance!

H2O(l)H2O(g)

NO+½ O2NO2

C2H6+O2CO2+H2O(g)

Accelerated ChemistryChapters 16 and 17 Worksheet #2Name ______

  1. Calculate the Heat of Reaction using Bond Energies:Don’t forget to balance!

HBrH2+Br2

CCl4+H2OCO2+HCl

C8H18+O2CO2+H2O

(over)

  1. Calculate the Heat of Reaction using Hess’ Law:Don’t forget to balance!

H2SO4H2O(g)+SO2+½ O2

NH3+O2NO+H2

C2H6+H2O(g)CO2+H2

Accelerated ChemistryChapters 16 and 17 Worksheet #3Name ______

  1. Calculate the Heat of Reaction using Bond Energies:

CH3OH+O2

C4H10+O2

  1. Calculate the Heat of Reaction using Hess’ Law:

C3H8(g) +NO(g)+ O2(g)3 CO(g) +NH3(g) + 2 ½ H2(g)

Acclerated ChemistryName ______

Chapters 16 and 17 Worksheet #4

1.According to the G equation, what combination of H and S always result in a spontaneous

reaction?

2.Explain the relationship between temperature and the spontaneity of reactions.

3.Based on the following values, calculate G values for each reaction and predict whether the

reaction will occur spontaneously at the indicated temperature:

a.A reaction with a H = 125 kJ/mol and S = 0.0350 kJ/mol K at 293 K

b.A reaction with a H =  85.2 kJ/mol and S = 0.125 kJ/mol K at 127 oC

c.A reaction with a H =  275 kJ/mol and S = 0.450 kJ/mol K at 500.0 oC

  1. The S for the reaction shown at 25.0 oC is 0.00300 kJ/mol K. Calculate the G for this reaction

and determine whether it will occur spontaneously at 25.0 oC.

C ( s ) + O2 ( g )CO2 ( g ) +393.51 kJ

5.When graphite reacts with H2 at 27.0 oC. H is  74.8 kJ/mol and S is  0.809 kJ/mol K.

Will this reaction occur spontaneously?

Accelerated ChemistryName ______

Chapters 16 and 17 Worksheet #5

  1. Draw a graph that displays an exothermic reaction. Label each axis, the activated complex, energy of activation, and Do the same for an endothermic reaction.
  1. Put the following chemicals in order from most to least stable (left to right):

ChemicalHeat of formation

XY- 65 kJ/mol

AB+79 kJ/mol

CD- 70 kJ/mol

FG+95 kJ/mol

  1. What are the differences between heat of reaction and heat of formation?
  1. If a reaction occurs where  = - 5.0 kCal and S = -0.350 kCal, calculate G and determine spontaneity at both negative and positive 250.0 Co.
  1. For the reaction3A+2B3C+2D

a)Write the rate law if it was a one step reaction

b)What would happen to the rate of reaction if [A] was doubled?

c)What would happen to the rate of reaction if [B] was tripled?

d)How many steps could you say the reaction had if the rate law was different than originally written.

  1. For the reactionA+B2C+Drate = k[A]3[B]2

a)What can you say about the number of steps in this reaction?

b)What happens to the rate if [A] is cut in half?

c)What happens to the rate if [B] is cut to 1/3 of the original amount?

  1. Explain the relationship between enthalpy, entropy, Gibbs free energy and the spontaneity of chemical reactions.