Answer:
At equilibrium the rate of the forward reaction is equal to the rate of the backward reaction.
When the product of a reaction at equilibrium is increased the equilibrium will shift left or to the reactant side. As a result the excess product will get converted to reactant. This is in accordance to Le Chatelier's principle.
Le Chatelier's principle states that when a system is subjected to stress the equilibrium will shift in a direction to minimize effect of the stress.
Thus the products added to the system at equilibrium will make the equilibrium shift to the reactant side, the rate of the reverse or backward reaction will increase.
Explanation:
Hope This Helps Amigo!
Answer:
a. 1,157x10⁻⁵M/s
b. 5,787x10⁻⁶M/s
Explanation:
For the reaction:
2H₂O₂(aq) → 2H₂O(l) + O₂(g).
a. The rate law of descomposition is:
Where d[H₂O₂] is the change in concentration of H₂O₂ (between 0s and 2,16x10⁴s) is (1,000M-0,500M) and dt is (0s-2,16x10^4s). Replacing:
As this rate is = d[O₂]/dt(Rate of production of O₂), the rate of production of O₂(g) is <em>1,157x10⁻⁵M/s</em>
b. Between 2,16x10⁴s and 4,32x10⁴s, rate law is:
The rates are <em>5,787x10⁻⁶M/s</em>
I hope it helps!
Answer:
2m.
Explanation:
molality = no.of moles of solute ÷ mass of solvent in kg
molalty = 1.5 moles ÷ 0.75 g
= 2m