<h2>The answer is option b "free energy is zero"</h2>
Explanation
- The reaction that has negative free energy are called exergonic reactions that means the reactants have more free energy than the product formed.
- The reaction that has positive free energy are called endergonic reactions that means the final state or the products formed have more free energy than the initial state or the reactants.
- The reaction that has zero free energy occurs when the free energy of both reactants and the products are same hence the rate of formation of products and reactants are equal.
- Therefore, when reactants and products are being formed at an equal rate the free energy is zero.
Answer:
D. The rate decreases as reactants are used up.
Explanation:
Initially, the rate increases until the reaction is at equilibrium. At equilibrium, the rate is constant.
As the reaction progresses, the rate decreases to zero when reactants are used up ( for irriversible reactions only )
I think ionic hope it helps
The oxidation state of Mn2 is 2+
For 1. 00 l of an aqueous buffer containing 60. 0 mmol of acetic acid (pa=4. 76) and 40. 0 mmol of acetate, the pH of this buffer is 4.58.
<h3>What is handerson Hasselbalch equation? </h3>
It is expressed as:
pH = pKa + log [A-]/[HA]
where,
[A-] is the molar concentration of conjugate base
[HA] is the molar concentration of weak acid
Given,
pKa = 4.76
<h3>Calculation of concentration:</h3>
C = n/V
= 60/1000
= 0.06M
C = 40/1000
= 0.04M
Now, substituting values in equation we get,
pH = 4.76 + log(0.04/0.06)
pH = 4.76 + (-0.176)
pH = 4.58
Thus by using Henderson Hasselbalch equation we find the value of pH of the buffer is 4.58.
learn more about pH :
brainly.com/question/9529394
#SPJ4
