The question is incomplete. Complete question is attached below.
Solution:
The reaction involved in present electrochemical cell is:
Mg(s) + Zn2+(aq.) ↔ Zn(s) + Mg2+ (aq.)
Thus, from above reaction it can be seen that 1 mole of Zn2+ produces 1 mole of Mg2+.
Thus,
2.5<span>
moles of Mg2+(aq) ions would be produced when 2.5 moles of Zn2+(aq) will react.</span>
A habitat must include all of the following except C. More than one population of a given species.
Answer:
.A catalyst provides an alternate mechanism for the reaction
Explanation:
The catalyst provides a mechanism of reaction having the lowest activation energy. It lowers the energy barrier between reactants and products hence it increases the rate of reaction by several orders of magnitude
We are given that the balanced chemical reaction is:
cacl2⋅2h2o(aq) +
k2c2o4⋅h2o(aq) --->
cac2o4⋅h2o(s) +
2kcl(aq) + 2h2o(l)
We known that
the product was oven dried, therefore the mass of 0.333 g pertains only to that
of the substance cac2o4⋅h2o(s). So what we will do first is to convert this
into moles by dividing the mass with the molar mass. The molar mass of cac2o4⋅h2o(s) is
molar mass of cac2o4 plus the
molar mass of h2o.
molar mass cac2o4⋅h2o(s) = 128.10
+ 18 = 146.10 g /mole
moles cac2o4⋅h2o(s) =
0.333 / 146.10 = 2.28 x 10^-3 moles
Looking at
the balanced chemical reaction, the ratio of cac2o4⋅h2o(s) and k2c2o4⋅h2o(aq) is
1:1, therefore:
moles k2c2o4⋅h2o(aq) = 2.28
x 10^-3 moles
Converting
this to mass:
mass k2c2o4⋅h2o(aq) = 2.28
x 10^-3 moles (184.24 g /mol) = 0.419931006 g
Therefore:
The mass of k2c2o4⋅<span>h2o(aq) in
the salt mixture is about 0.420 g</span>
