Reaction Spontaneity
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Transcript of Reaction Spontaneity
Reaction Spontaneity
How can a fire start on its own? (without a spark)
Spontaneous Reaction
• Occurs naturally and favors formation of products
4Fe(s) + 3O2(g) 2Fe2O3(s) ΔH = -1625 kJ
CH4(g) + 2O2(g) CO2(g) + 2H2O(l) ΔH = -891 kJ
Nonspontaneous Reaction
Does not favor formation of products
2Fe2O3(s) 4Fe(s) + 3O2(g) ΔH = 1625 kJCO2(g) + 2H2O(l) CH4(g) + 2O2(g) ΔH = 891 kJ
H2O(s) H2O(l) ΔH = 6.01 kJ
Some endothermic reactions are SPONTANEOUS!
ENTROPY (S)
• The measure of disorder or randomness of particles in a system
LAW OF DISORDERSpontaneous processes always increase the entropy of a system
Law of Disorder
Changes in Entropy (ΔS)
•Δssystem = Sproducts – Sreactants
1. Changes in State
2. The dissolving of a gas in a solvent always results in a decrease in entropy.
CO2(g) CO2(aq) Δssystem < 0
3. Assuming no change in physical state, the entropy increases when: # of product particles > # of reactant particles.
2SO3(g) 2SO2(g) + O2(g) Δssystem > 0
4. when a solid or a liquid dissolves to form a solution.
NaCl(s) Na+(aq) + Cl-(aq) Δssystem > 0
5. increase in the temperature increase in entropy
Does entropy increase or decrease?
CaCO3 (s) CaO (s) + CO2 (g)
NH3 (g) + HCl (g) NH4Cl (s)
How ΔHsystem and ΔSsystem
affect reaction spontaneity
ΔH ΔS Spontaneous?
- + yes+ + Depends on T- - Depends on T+ - No
Gibb’s Free Energy!!
ΔGsystem = ΔHsystem – TΔSsystem
The energy that is available to do work (useful energy)
ΔGsystem and reaction spontaneity
Type of Reaction or Process
ΔGsystem ΔSuniverse
Spontaneous - +Nonspontaneous + -
Is the following reaction spontaneous?
N2(g) + 3H2(g) 2NH3(g) ΔH°system= -91.8 kJ
ΔS°system= -197 J/K
ΔGsystem = ΔHsystem – TΔSsystem
For a process, ΔHsystem=145 kJ and ΔSsystem=322J/K. Is the reaction spontaneous at 382 K?