1) From the texts below do what you ask. A) Atmospheric nitrogen dioxide acts as
ID: 522521 • Letter: 1
Question
1) From the texts below do what you ask.
A) Atmospheric nitrogen dioxide acts as the catalyst for the oxidation reaction of sulfur dioxide in sulfur trioxide by atmospheric oxygen. The latter forms sulfuric acid by reacting with water.
Fully represent, solid, liquid, gaseous or aqueous, the chemical equations of the above reactions.
B) Describe some physical characteristics that allow to identify experimentally ionic substances
C) N 2 (g) + 3 H 2 (g) -----> 2 NH 3 (g)
From the beginning of Le Châtelier, describe the procedures that could be adopted to shift the equilibrium of the above reaction
In order to increase the amount of NH 3 (g) formed.
D) Describe the main characteristics of the reaction represented by the graph below.
E) Considering that the pH of the pure water is equal to 7.0 and based on the self-dissolution equation H2O (l) --------> H3O + (aq) + OH- (aq), show That the ionic product constant of water, Kw, is equal to 1.0 × 10 -14.
complexo ativado evolucao da reacaoExplanation / Answer
A:
2 SO2 (g) + O2 (g) <-----> 2 SO3 (g)
2 SO3 (g) + 2 H2O (l) ---> 2H2SO4 (l)
B: some physical characteristics that allow to identify experimentally ionic substances.
C: N2 (g) + 3 H2 (g) -----> 2 NH3 (g)
Inorder to increase the amount of NH3 formed i.e to shift the equilibrium reaction in forward direction.
increse the concentration of N2 and H2 and according to lechatlier's principle the reaction will move in forward direction.
D: Energy of product is less than energy of reactant. Thus, in the net reaction there is the release of energy. Hence, it is an exothermic reaction.
E: pH of pure water = 7
- log[H+] = 7
[H+] = 10-7
pH +pOH =14
pOH =7
to show :Kw= 1.0 x 10¹
H2O (l) --------> H3O + (aq) + OH-
Kw = [H3O+ ] [OH-]
= 10-7 * 10-7 = 10-14
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