I need to know all of those questions please help
1 answer:
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Answer:
The answer is 2.03
Explanation:
The pH of a solution can be found by using the formula
where H+ is the Hydrogen ion concentration
From the question we have
We have the final answer as
<h3>2.03 </h3>Hope this helps you
C. Aluminum (Al) oxidized, zinc (Zn) reduced
<h3>Further explanation</h3>Given
Metals that undergo oxidation and reduction
Required
A galvanic cell
Solution
The condition for voltaic cells is that they can react spontaneously, indicated by a positive cell potential.
or:
E ° cell = E ° reduction-E ° oxidation
For the reaction to occur spontaneously (so that it E cell is positive), the E° anode must be less than the E°cathode
If we look at the voltaic series:
<em>Li-K-Ba-Ca-Na-Mg-Al-Mn- (H2O) -Zn-Cr-Fe-Cd-Co-Ni-Sn-Pb- (H) -Cu-Hg-Ag-Pt-Au </em>
The standard potential value(E°) from left to right in the voltaic series will be greater, so that the metal undergoing an oxidation reaction (acting as an anode) must be located to the left of the reduced metal (as a cathode)
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From the available answer choices, oxidized Al (anode) and reduced Zn (cathode) are voltaic/galvanic cells.
Answer:
Value of equilibrium constant is 0.0888
Explanation:
Both and
are gaseous. Hence equilibrium constant depends upon partial pressures of
and
.
Initially no and
were present.
Hence mole fraction of and
at equilibrium can be calculated from coefficient of
and
in balanced equation.
Mole fraction of = (number of moles of
)/(total number of moles of
and
) =
Mole fraction of = (number of moles of
)/(total number of moles of
and
) =
Let's assume both and
behaves ideally.
Therefore partial pressure of ,
and P_{CO_{2}}= x_{CO_{2}}.P_{total}
Where x represents mole fraction
So,
So,