A.) Q < K because Q decreased
B. shift right
K = Product/Reactant
An endothermic reffers to any reaction which absorbs energy from its surroundings, usually in the form of heat.
ΔH. In endothermic reactions, K increases when Temperature increases.
The given reaction is an endothermic reaction, and in an endothermic reaction, when there is increase in temperature, the product side is more favored. The system will shifts to the right side of the reaction. Q < K then K is constant and Q is decreased.then Q < K because Q decreased
The system respond to a temperature increase by shifting to the right
Q < K because K increased
The system will SHIFT TO THE RIGHT
First, the reaction is endothermic. That is, a reaction in which heat is absorbed from the surroundings. ΔH is positive for endothermic reactions.
At the addition of temperature, the system absorbed more heat causing more products to be formed, shifting the equilibrium to the right.
The equilibrium constant k will therefore increase as the concentration of product increases
K = [B] / [A].
Q < K because K increased.
Reaction equilibrium shift towards right.
For this reaction, is positive. This signifies that the given reaction is endothermic. So, with increase in temperature, reaction equilibrium shift towards right in accordance with Le-chatelier principle.
So, with increase in temperature, more A will be converted to B.
Equilibrium constant in terms of concentration, where [B} and [A} are equilibrium concentrations of B and A respectively.
Hence will increase with increase in temperature.
At equilibrium, Q (reaction quotient) = .
But immediately after an increase in temperature, Q < as is higher in this increased temperature as compared to previous temperature.
When equilibrium is re-established the value of K will be greater. Temperature changes are the only changes that actually change the value of K.