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
M(Mn(ClO3)3)=(54.938)+(35.45x3)+(15.999x9)
M(Mn(ClO3)3)=305.279 g/mol
Answer:
1.3 mol H₂O
Explanation:
Let's consider the decomposition reaction of ammonium perchlorate.
NH₄ClO₄(s) → 1/2 N₂(g) + 1/2 Cl₂(g) + O₂(g) + 2 H₂O(g)
As we can see in the balanced equation, the molar ratio of ammonium perchlorate to water is 1:2. The moles of water produced by the reaction of 2.5 mol of ammonium perchlorate.
2.5 mol NH₄ClO₄ × (2 mol H₂O / 1 mol NH₄ClO₄) = 1.3 mol H₂O
Answer:
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