If we analyze the situation analytically, there are situations or states. Then, we are also given with 2 values of pressure and 1 value of volume. Lastly, temperature was set as constant. Thus, this means we use the Boyle's Law.
P₁V₁ = P₂V₂
Let's find V₂.
(1 atm)(1.72 L) = (35 atm)(V₂)
Solving for V₂,
<em>V₂ = 0.049 L</em>
Au³⁺ metal ion is reduced in the Au/Cr cell and Co²⁺ metal ion is reduced in the Co/Zr cell
<h3>What is a voltaic cell?</h3>
A voltaic cell is a cell that generates electricity by a spontaneous redox reaction.
It is an electrochemical cell, also known as a galvanic cell and
Electrical energy is created by converting chemical energy.
Examples of voltaic cells include the dry cell, nickel-cadmium cell, lead storage cell, and fuel cells.
The half-cell reactions for each cell are given by
; E° = 1.50 V
; E° = –0.74 V
; E° = –0.28 V
E° = –0.76 V
Thus, Au³⁺ is reduced in the Au/Cr cell and Co²⁺ is reduced in the Co/Zr cell
Learn more about Voltaic cell:
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Answer:
A chemical bond is defined as the force which helps to bind more than two atoms in a molecule. There are different types of chemical bonding are present in molecules such as:
1) Ionic bonding: Because of the transfer of electrons it is present in ionic compounds. BaS is an example of ionic bonding which is containing some covalent character.
2) Covenant bonding: Because of the sharing of electrons it forms molecules. Rubber is the example of covalent bonding with some van der walls.
3) Metallic bonding: In the free state it is present in atoms of metal such as Brass is a good example of a metallic bonding because it is a metal alloy.
4) Van der walls bonding: In atoms, It includes repulsion and attraction. Solid xenon is the example of Van der wall bonding because it is an inert gas.
When the neutrons and electrons are the same. For example, sodium (Na) has an atomic mass of 11, meaning it has 11 protons and 11 electrons etc.
PV
= nRT
We
are solving for pressure. We are given the volume, which is 0.100 L (equivalent
to 100 mL). The temperature is 273.15 K (equivalent to 0 Celsius). All we need
to do is convert the grams to moles before we can solve for pressure.
N₂
has a molecular mass of 28.02. This means that 510 g N₂ * (1 mole N₂/28.02 g
N₂) = 18.2 moles N₂
PV
= nRT
P
= nRT/V
R
is the gas constant. R = 0.08206 atm*L/(K*mol)
P
= (18.2 mol)*(0.08206 atm*L/(K*mol))*(273.15 K) / (0.100 L)
<span>P
= 4.08 *10^3 atm</span>
<span>
</span>
<span>The pressure is 4.08*10^3 atm.</span>
