10.102 Ammonia can react with oxygen gas to form nitrogen dioxide and water. (a) Write a balanced chemical equation for this reaction. (b) Use tabulated data to determine the free energy change for the reaction and comment on its spontaneity. (c) Use tabulated data to calculate the enthalpy change of the reaction, (d) Determine how much heat flows and in what direction when 11.4 g of ammonia gas is burned in excess oxygen.
Interpretation:
Ammonia reacts with Oxygen gas to form Nitrogen dioxide and water. The feasibility of this reaction can be identified by using free energy change. The free energy change, enthalpy change and entropy change can be calculated by using standard data.
Concept introduction: The free energy change of the reaction
If the sign of the free energy change is negative, it indicates that the reaction is spontaneous.
Answer to Problem 10.102PAE
Solution: a) The balanced equation is
b)
c)
d) The amount of heat produced by 11.4 g of NH3 = 233.88 kJ
Given:
From the standard data −
Explanation of Solution
a)
The balanced chemical equation of the given reaction is as follows.
b) From the standard data −
As
c)
From the standard data −
d)
From the balanced equation, 4 mols
Therefore, the amount of heat produced by 11.4 g of ammonia
As the above value is in negative, we conclude that the reaction is exothermic. Hence heat transfers to surroundings.
The given reaction is spontaneous as free energy change of the reaction is negative. The given reaction is an exothermic reaction as enthalpy change is negative and it produces 1397.56 kJ of energy.
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