The equilibrium constant of a reaction is defined as:
"The ratio between equilibrium concentrations of products powered to their reaction quotient and equilibrium concentration of reactants powered to thier reaction quotient".
The reaction quotient, Q, has the same algebraic expressions but use the actual concentrations of reactants.
To solve this question we need this additional information:
<em>For this reaction, K = 6.0x10⁻² and the initial concentrations of the reactants are:</em>
<em>[N₂] = 4.0M; [NH₃] = 1.0x10⁻⁴M and [H₂] = 1.0x10⁻²M</em>
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Thus, for the reaction:
N₂ + 3H₂ ⇄ 2NH₃
The equilibrium constant, K, of this reaction, is defined as:
And Q, is:
Where actual concentrations are:
[NH₃] = 1.0x10⁻⁴M
[N₂] = 4.0M
[H₂] = 2.5x10⁻¹M
Replacing:
As Q < K,
<h3>The chemical system will shift to the right in order to produce more NH₃</h3>Learn more about chemical equililbrium in:
Answer:
Explanation:
As energy is absorbed therefore it is an endothermic reaction. Hence energy value should be written in the product side with a negative sign.
Reaction:
C balance:
H and O balance:
Here 2 moles of react. So, energy absorbed during the reaction is
kJ or 46.6 kJ
Energy balance:
Balanced thermochemical equation:
Answer:
Explanation:
Assuming that temperature is constant
According to Boyle's Law, at constant temperature pressure is inversly proportional to the volume and mathematically it can be expressed as:
..........1
from the first equation after putting all the value
we get,