Answer:
Explanation:
Hello,
a) In this case, since the heat associated with the dissolution of ammonium nitrate is positive, such reaction is endothermic as it absorbs heat.
b) Now, for computing the temperature once the dissolution is done, we apply (considering that it is a cooling process):
Nonetheless, we should first compute the moles of the mixture as:
Thus, the total absorbed heat is:
Now, the temperature is:
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Answer:
Explanation:
The atomic weight of oxygen = 15.9994 g
This mass corresponds to 1 mole of the oxygen atoms.
Thus,
15.9994 g mass of oxygen contains atoms of oxygen.
1.4 kg = 1400 g ( 1 kg = 1000 g)
So,
1400 g mass of oxygen contains atoms of oxygen.
Number of atoms in 1400 g of oxygen =
Also, 1 atom of oxygen contains 8 protons
Charge of 1 proton = +
So, Charge on 1 atom of oxygen =
Thus,
Charge on atoms of oxygen =
Thus, positive charge in 1.4 kg of oxygen =
Answer:
1.930 * 10⁻⁹ mg of Mn⁺² are left unprecipitated.
Explanation:
The reaction that takes place is:
Mn⁺² + S⁻² ⇄ MnS(s)
ksp = [Mn⁺²] [S⁻²]
If the pksp of MnS is 13.500, then the ksp is:
From the problem we know that [S⁻²] = 0.0900 M
We use the ksp to calculate [Mn⁺²]:
3.1623*10⁻¹⁴= [Mn⁺²] * 0.0900 M
[Mn⁺²] = 3.514 * 10⁻¹³ M.
Now we can calculate the mass of Mn⁺², using the volume, concentration and atomic weight. Thus the mass of Mn⁺² left unprecipitated is:
3.514 * 10⁻¹³ M * 0.1 L * 54.94 g/mol = 1.930 * 10⁻¹² g = 1.930 * 10⁻⁹ mg.