If more acetic acid were added to a solution at equilibrium, [H⁺] and [CH₃CO₂⁻] would increase to counteract the perturbation. (Option C)
<h3>How do systems at equilibrium respond to perturbation?</h3>
When a system at equilibrium suffers a perturbation, it shifts its equilibrium position to counteract such perturbation.
Let's consider a solution of acetic acid at equilibrium.
CH₃CO₂H(aq) = CH₃CO₂⁻(aq) + H⁺(aq)
If more acetic acid were added to the solution, the system will shift toward the products to counteract such an increase.
How would the system change if more acetic acid were added to the solution?
A. [H⁺] would decrease and [CH₃CO₂⁻] would increase. NO.
B. [H⁺] and [CH₃CO₂⁻] would decrease. NO.
C. [H⁺] and [CH₃CO₂⁻] would increase. YES. Both products would increase.
D. [H⁺] would increase and [CH₃CO₂⁻] would decrease. NO.
If more acetic acid were added to a solution at equilibrium, [H⁺] and [CH₃CO₂⁻] would increase to counteract the perturbation.
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Water will have higher surface tension.
Explanation:
There are strong hydrogen bonds and strong intermolecular forces present in water. Water is polar in nature that is why surface tension is present in it. The force of attraction between the particles is the main factor for surface tension.
The cohesion force in the liquid causes surface tension.
Since the other substance is acetone which does not form strong intermolecular forces hence it has low value of surface tension. They have low cohesive forces and get stick to the surface and are spilled instead of attaining minimal volume.
I think the answer is Density
The system is not at equilibrium.
The reaction will proceed to the right to attain the equilibrium.
Let's consider the following reaction.
2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)
The pressure equilibrium constant (Kp) is 60.6. To determine if the system is at equilibrium when the pressure of each component is 1.75 atm, we have to calculate the reaction quotient (Q) and compare it with Kp.
Q = [NO]².[Br₂] / [NOBr]²
Q = (1.75)².(1.75) / (1.75)²
Q = 1.75
Since Q ≠ Kp, the system is not at equilibrium.
Since Q < Kp, the reaction will proceed to the right to attain the equilibrium.
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Answer: Empirical formula of this compound is
Explanation:
Mass of Cr= 104.0 g
Mass of O = 48.0 g
Step 1 : convert given masses into moles.
Moles of Cr =
Moles of O =
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For Cr =
For O =
Converting into simple whole number ratios by multiplying by 2
The ratio of Cr : O= 2: 3
Hence the empirical formula is
The most likely empirical formula of this compound is