Answer:
Chemical formula is CoCl. 3H₂O
Explanation:
Data Given
Percentage of water = 45.43%
Percentage of CoCl. = 54.57%
Chemical Formula of the hydrates = ?
Solution:
First, find the mass of each of the part ( CoCl and water) in 100 g of the Compound.
Mass of CoCl = 28 + 35.5
Mass of CoCl = 63.5
Mass of H₂O = 18 g
Now find how many moles are there for each element in 100 g of compound
So,
The percentage will be count in grams for 100g in compound
Find the moles in total compounds
Formula Used for CoCl
mole of CoCl = mass of CoCl / Molar mass of CoCl
mole of CoCl = mole of 54.57 g / 63.5 g/mol
mole of CoCl = 0.859
Formula Used for H₂O
mole of H₂O = mass of H₂O/ Molar mass ofH₂O
mole of H₂O = 45.43 g / 18 g/mol
mole of H₂O = 2.539
Now
To find the Chemical formula
Divide each one by the smallest number of moles
CoCl = 0.859 / 0.859
CoCl = 1
For H₂O
H₂O = 2.539 / 0.859
H₂O = 3
Multiply the mole fraction to a number to get the whole number.
CoCl = 1
H₂O = 3
So,
The Chemical formula is CoCl. 3H₂O
Answer:
A option is correct.
(a) Energy can create a change.
Explanation:
Diagram A shows the Lewis structure (LS) of CH_2O. The formal charge on each atom is zero.
To get the formal charge (FC) on the atoms, cut each bond in half, as in <em>Diagram B</em>. Each atom gets the electrons on its side of the cut.
Formal charge = valence electrons in isolated atom - electrons on bonded atom
FC = VE - BE
<em>On O:
</em>
VE = 6
BE = 2 lone pairs 2 + 2 bonding electrons = 4 + 2 = 6
FC = 6 – 6 = 0.
<em>On H:
</em>
VE = 1
BE = 1 bonding electron
FC = 1 – 1 = 0
<em>On C:
</em>
VE = 4
BE = 1 in each single bond + 2 in the double bond = 2 + 2 = 4
FC = 4 - 4 = 0
Answer:
it will dilute to its natrual state. so c
Explanation:
