a because as temperature increases, reaction rate increases.
When an atom gains an electron it becomes a negatively charged ion. When an atom looses an electron it becomes positively charged because the number of positively charged protons.
Hope this helps
<h2>Answer:</h2>
<u>Decreasing Ionization energy</u>
<h2>Explanation:</h2>
As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to increasing radius and increasing shielding effect. In other words when we move to the right of a period, the number of electrons increases and the strength of shielding increases. As a result, it is easier for valence shell electrons to ionize, and thus the ionization energy decreases down a group.
<u>Answer:</u> The standard potential of the cell is 0.77 V
<u>Explanation:</u>
We know that:
The substance having highest positive 
reduction potential will always get reduced and will undergo reduction reaction.
The half reaction follows:
<u>Oxidation half reaction:</u> 
<u>Reduction half reaction:</u> 
( × 2)
To calculate the 
of the reaction, we use the equation:
Substance getting oxidized always act as anode and the one getting reduced always act as cathode.
Putting values in above equation follows:
Hence, the standard potential of the cell is 0.77 V
Answer:
Henderson Hasselbalch equation: pH = pKa + log [salt]/[acid]
You need to know the pKa for acetic acid. Looking it up one finds it to be 4.76
(a). pH = 4.76 + log [0.13]/[0.10]
= 4.76 + 0.11
= 4.87
(b) KOH + CH3COOH =>H2O + CH3COOK so (acid)goes down and (salt)goes up. Assuming no change in volume, you have 0.10 mol acid - 0.02 mol = 0.08 mol acid and 0.13 mol salt + 0.02 mol = 0.15 mol salt
pH = 4.76 + log [0.15]/[0.08]
= 4.76 + 0.27
= 5.03
