Red is the color that its related to
Answer:
(A) first order reaction
Explanation:
A first order reaction is a type of reaction in which the rate of the reaction depends only on the concentration on one of the reactants. Since A is the only reactant we have, it is right to deduce that this reaction is a first order reaction.
Note: while the order of this reaction is 1, its molecularity is 2. The molecularity of a reaction is the number of moles of reactants that is actually reacting.
(B) is wrong
This is because a zero order reaction is one in which the rate of reaction is not influenced by the concentrations of the reactants and hence remains constant irrespective. Since we were not furnished with this idea in the question, it is only right that we reject this answer.
(C) is wrong.
C is outrightly wrong as we have only one reactant.
(D) is wrong
We have only one reactant.
Cytosine (C) and Guanine (G) are more steady under expanding heat since C and G have three hydrogen bonds while Adenine (An) and Thymine (T) have just two. The more hydrogen bonds there are, the more steady the nucleotides are. More bond dependability requires more warmth vitality to separate the securities, and since G≡C have more hydrogen securities than A=T, they are thusly more steady under expanding heat.
The decomposition reaction of hydrogen peroxide:
2 H₂O₂(aq) → 2 H₂O(l) + O₂(g)
The order of reaction is : first order reaction.
[H₂O₂]₀ = 12 M at time = 0
[H₂O₂] = 9.5 M at time = 30 minutes
Average reaction rate = - (Δ[reactants] / Δt)
= - (final reactants conc. - initial reactants conc.) / Δt
= - (9.5 M -12 M) / (30 min - 0 min)
= 0.083 mol / L.min
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