If the concentration of the product NH3 was increased from 1.0 x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and
1 answer:
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
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Answer:
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
Order of the reaction is defined as the sum of the concentration of terms on which the rate of the reaction actually depends. It is the sum of the exponents of the molar concentration in the rate law expression.
For reactions which takes place in multiple steps are complex reactions and the order is given by the slowest step which is the rate limiting step.
For the given reaction, the rate limiting step is
Rate law will be ,