True, I’m sorry if I’m wrong
Answer:
Part A: 2N₂O(g) ⇄ 2N₂(g) + O₂(g)
Part B: -r = K*[N₂O]²
Part C: K= k1*k2
Explanation:
Part A
To do the balance chemical question for the overall chemical reaction, we must sum the reaction of the steps, eliminating the intermediaries, which are the compounds that have the same amount both at reactants and products (bolded).
N₂O(g) ⇄ N₂(g) + O(g)
N₂O(g) + O(g) ⇄ N₂(g) + O₂(g)
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2N₂O(g) + O(g) ⇄ 2N₂(g) + O(g) + O₂(g)
2N₂O(g) ⇄ 2N₂(g) + O₂(g)
Part B
The velocity of the reaction (r) can be calculated based on the reactants or based on the products. Let's do it based on the disappearing of the reactant. Because it is disappearing, the variation at its concentration must be negative, so the rate will be negative.
Let's suppose its an elementary reaction, so, the concentration of the reactant must be elevated by its coefficient. And let's call the overall rate constant as K:
-r = K*[N₂O]²
Part C
Because the steps were summed, and the reactions were not multiplied by a constant or inverted, the constant K is just the multiplication of the constants of the steps:
K= k1*k2
Ionization is a formation of ions from neutral atoms or molecules.
SO₂ + H₂O = HSO₃⁻ + H⁺
Mg(OH)₂ = Mg²⁺ + 2OH⁻
The volume of O₂ : 21 L
<h3>Further explanation</h3>
Given
8.7 grams of C₂H₄
Required
Volume O₂
Solution
Reaction
C₂H₄ + 3 O₂ ⇒ 2 CO₂ + 2 H₂O
mol C₂H₄(MW= 28 g/mol) :
= mass : MW
= 8.7 g : 28 g/mol
= 0.311
From the equation, mol O₂ :
= 3/1 x mol C₂H₄
= 3/1 x 0.311
= 0.933
At STP, 1 mol gas=22.4 L, so for 0.933 mol :
= 0.933 x 22.4 L
= 20.899 L ≈ 21 L
