Correct Answer: option <span>(1) Mn(s)
Reason:
The </span><span>spontaneity of electrochemical cell, depends on the it's Eo value. Electrochemical cells with positve Eo are spontanous and vice-versa.
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In present case, the Eo of half-cell of interest are as follows:
Eo Zn2+/Zn = <span>-0.763v
</span>Eo Mg2+/Mg = 2.37v
Eo Mn2+/Mn = -1.18v
Therefore, Eo cell (with Zn as one of the half-cell) = Eo Zn2+/Zn - Eo Mn2+/Mn
= -0.763 - (-1.18)
= 0.417v
On other hand, Eo cell (with Mg as one of the half-cell) = Eo Mg2+/Zn - Eo Mn2+/Mn
= -2.37 - (-1.18)
= -1.19v
Thus, Mn(s) <span>metal will spontaneously react with Zn2+(aq), but will not spontaneously react with Mg2+(aq)</span>
We need to first come up with a balanced equation:
→
We know that the molar ratio of hydrogen to oxygen to water now is 4:1:2.
Converting the amount of grams given to moles is as follows:
Hydrogen:
Oxygen:
We know now that the limiting reactant is oxygen. We can then know that the number of moles of water are produced are double the number of moles of oxygen used due to the ratio that we established at the beginning - 4:1:2.
So we now can use 6.25 moles of water as the amount produced.
Then we convert moles of water to grams:
Now we know that there are 112.59g of water produced when we start with 50g of hydrogen and 50g of water.
Answer:
a) 1:1
Explanation:
By the ideal gas law:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is temperature.
Both ballons are at the same conditions, so the gases have the same temperature and pressure. The number of moles is the mass(m) divided by the molar mass (Mr). The molar masses are:
Mr(Ne) = 20 g/mol
Mr(Ar) = 40 g/mol
Calling 1 for Ne, and 2 for Ar:
P1*V1 = (m1/20)*R*T1
m1 = 20P1V1/RT1
P2*V2 = (m2/40)*R*T2
m2 = 40P2V2/RT2
V1 = 2V2
m1/m2 = (20P1V1/RT1)/(40P21V2/RT2)
P1 = P2, T1 =T2 so they can be canceled, such as the R:
m1/m2 = 20V1/40V2
m1/m2 = 20*2V2/40V2
m1/m2 = 40V2/40V2
m1/m2 = 1/1
m1:m2 = 1:1