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poniatowski23
06.07.2019 •
Chemistry
Xenon (xe) of mass 5.08 g reacts with fluorine to form 9.49 g of a xenon fluoride compound. what is the empirical formula of this compound?
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Ответ:
mass of Xenon (Xe) = 5.08 g
mass of Fluorine (F) = 9.49 g - 5.08 g = 4.41 g
Determine the number of moles of each of the element in the compound.
moles of Xenon (Xe) = (5.08 g)(1 mol Xe / 131.29 g of Xe) = 0.0387 mols of Xe
moles of Fluorine (F) = (4.41 g)(1 mol F/ 19 g of F) = 0.232 mols of F
The empirical formula is therefore,
Xe(0.0387)F(0.232)
Dividing the numerical coefficient by the lesser number.
XeF₆
Ответ:
Approximately
.
Explanation:
Balance the equationTo balance this equation, start by setting the coefficient of the most complex species to
. For example,
has more atoms in each of its formula unit than any other species in this reaction. Let the coefficient of
That formula unit of
would include:
The other product,
, contains neither
atoms nor
atoms. Therefore, the product side would include exactly
oneAtoms are conserved in a chemical reaction. The reactant side shall also include:
Among the reactants,
is the only source of
atoms. Each formula unit of
Similarly, the coefficient of
would be
.
There would be exactly![2](/tpl/images/0629/7968/05229.png)
atom on the reactant side (from
.) The products should also include
Hence the equation:
.
Calculate n(Cu(NO₃)₂ (aq))The ratio between the coefficients of
and
is:
Rearrange this equation to obtain:
In other words,
(the number of moles of
that is produced) can be found from
(the number of moles of
that is produced.)
On the other hand,
can be found from
(the mass of
that is produced) using
(the formula mass of
.)
Look up relative atomic mass data of
on a modern periodic table:
Therefore, the relative atomic mass of
would be:
Calculate
:
Calculate
: