When the reactants have less enthalpy than the products, then __________. A. heat energy is given out B. None of these C. heat e
1 answer:
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The chemical system will shift to the left in order to produce more N₂ , H₂.
The missing data in the question is
The equilibrium constant (K) of the reaction below is K = 6.0 x 10⁻² with initial concentrations as follows: H₂ = 1.0 x 10⁻² M, N₂ = 4.0 M, and NH₃ = 1.0 x 10⁻⁴M.
<h3>What is Chemical Equilibrium?</h3>When the rate of forward reaction is equal to the rate of the backward reaction then the equation is said to be in Chemical Equilibrium.
N₂ + 3H₂ --> 2NH₃
The reaction quotient, Q, has the same algebraic expressions but uses the actual concentrations of reactants.
[N₂] = 4.0M; [NH₃] = 1.0x10⁻⁴M and [H₂] = 1.0x10⁻²M
Thus, for the reaction:
N₂ + 3H₂ ⇄ 2NH₃
The equilibrium constant, K, of this reaction, is defined as:
Q = (5.6 x 10⁻³ )² / (1.0 x 10⁻²) ³(4.0 )
Q = 7.84
As Q > K,
The chemical system will shift to the left in order to produce more N₂ , H₂
To know more about chemical equilibrium
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Answer:
See picture below
Explanation:
You are not providing the starting compound. However, I found a similar question so, I will draw the product of this compound, and then, you follow the same procedure.
As the problem states, the diazomethane is often used in reaction with carboxilic acid. This kind of reaction will do an esterification reaction, and the final product will always result in an esther.
So, with the example I give you here, all you have to do is replace the OH in the carboxilic group of your initial compound, for the OCH₃ group.
See picture below.
Hope this helps
