Milk is a complex colloidal system.
Answer:
.
Explanation:
Electrons are conserved in a chemical equation.
The superscript of
indicates that each of these ions carries a charge of
. That corresponds to the shortage of one electron for each
ion.
Similarly, the superscript
on each
ion indicates a shortage of three electrons per such ion.
Assume that the coefficient of
(among the reactants) is
, and that the coefficient of
(among the reactants) is
.
.
There would thus be
silver (
) atoms and
aluminum (
) atoms on either side of the equation. Hence, the coefficient for
and
would be
and
, respectively.
.
The
ions on the left-hand side of the equation would correspond to the shortage of
electrons. On the other hand, the
ions on the right-hand side of this equation would correspond to the shortage of
electrons.
Just like atoms, electrons are also conserved in a chemical reaction. Therefore, if the left-hand side has a shortage of
electrons, the right-hand side should also be
electrons short of being neutral. On the other hand, it is already shown that the right-hand side would have a shortage of
electrons. These two expressions should have the same value. Therefore,
.
The smallest integer
and
that could satisfy this relation are
and
. The equation becomes:
.
Answer:
The enthalpy of combustion of ethanol in kJ/mol is -1419.58 kJ/mol.
Explanation:
The heat absorbed by the bomb and water is equal to the product of the heat capacity and the temperature change. Working with this equation, and assuming no heat is lost to the surroundings, we write
:
qcal= Ccal × ΔT= 490 J/K × 276.7 K= <u>135,583 J</u> = 135.58 kJ
Note we expressed the temperature change in K, because the heat capacity is written in K.
<u>
Now that we have the heat of combustion, we need to calculate the molar heat. </u>
Because qsystem = qrxn + qcal and qrxn = -qcal, the heat change of the reaction is -135.58 kJ.
This is the heat released by the combustion of 4.40 g of ethanol ; therefore, we can write the <u>conversion factor as 135.58 kJ/ 4.40 g</u>.
The molar mass of ethanol is 46.07 g, so the heat of combustion of 1 mole of ethanol is
:
molar heat of combustion= -135.58 kJ/4.40 g x 46.07 g/ 1 mol= -1419.58 kJ/mol
Therefore, the enthalpy of combustion of ethanol in kJ/mol is -1419.58 kJ/mol.
Answer:
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