(a)
Interpretation:
Enthalpy change for each reaction has to be calculated.
Concept Introduction:
Hess's Law:
The enthalpy change of given reaction is calculated by subtraction of sum of enthalpy of formation reactants from sum of enthalpy of formation reactant products.
(b)
Interpretation:
The exothermic and endothermic reaction has to be given for below given reactions.
Concept Introduction:
In the
(c)
Interpretation:
The reaction, which contains greater entropy, has to be given from below given reactions.
Concept Introduction:
If number of mole increases result the increasing entropy value and decreases result the decreasing entropy of reaction.
(d)
Interpretation:
The reaction, which is favor at low temperature, has to be given from below given reactions.
Concept Introduction:
If number of mole increases result the increasing entropy value and decreases result the decreasing entropy of reaction.
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Chemistry: The Molecular Science
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- Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) 2 H2O(g) + O2(g) (b) CO(g) + O2g CO2(g) (c) C(s) + CO2(g) 2 CO(g) (d) NiO(s) + CO(g) Ni(s) + CO2(g)arrow_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardSuppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forward
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