The data table below shows four different chemical reactions, the temperature change of each, and the duration of the change in
2 answers:
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Answer:
The molarity of the solution = 0.1895 M
Explanation:
The mass of the obtained = 10.55 g
Molar mass of = 278.1 g/mol
The formula for the calculation of moles is shown below:
Thus,
From the reaction:-
1 mole of is produced from 1 mole of
Also,
0.0379 mole of is produced from 0.0379 mole of
Mole of = 0.0379 mol
Volume = 200.0 mL = 0.2 L ( 1 mL = 0.001 L )
Molarity is defined as the number of moles present in one liter of the solution. It is basically the ratio of the moles of the solute to the liters of the solution.
The expression for the molarity, according to its definition is shown below as:
Thus,
<u>The molarity of the solution = 0.1895 M</u>
Answer:
This ion is in an octahedral geometry.
See the diagram attached for the Lewis Dot Structure of the iodide hexafluoride cation . (Created with Google Drawings.)
Note that in this diagram,
- A pair of double dots on an atom represent a lone pair of electrons.
- A single dash represents a single chemical bond.
- The square bracket and the superscript indicates that this structure is charged.
Explanation:
The iodine in forms an expanded octet. There are twelve valence electrons in total around this atom.
- Each of the six fluorine atom needs 8 - 7 = 1 electron to achieve an octet of eight electrons.
- The iodine atom needs 12 - 7 = 5 electrons to achieve an expanded octet of twelve electrons.
- The ion carries a positive charge of +1. Atoms in this ion lacks one extra electron.
Overall, there needs to be more electrons for seven atoms to achieve an octet. They will form half that number of chemical bonds. That's
bonds.
Now consider: what will be the geometry of this ion? There are six chemical bonds but no lone pair around the central iodine atom. The six bonds repel each other equally. They will stay as far apart from each other as possible. As a result, the shape of the ion will be octahedral. Each of the fluorine atoms occupies a vertex.
