The empirical formula is C₇H₆O₂.
Assume that you have 100 g of the compound.
Then you have 68.84 g C and 4.962 g H.
Mass of O = (100 – 68.84 – 4.962) g = 26.20 g O.
Now, we must convert these masses to moles and find their ratios.
From here on, I like to summarize the calculations in a table.
<u>Element</u> <u>Mass/g</u> <u>Moles</u> <u>Ratio</u> <u> ×2</u> <u>Integers</u>
C 68.84 5.732 3.501 7.001 7
H 4.962 4.923 3.006 6.012 6
O 26.20 1.638 1 2 2
The empirical formula is C₇H₆O₂.
Answer:
768g
Explanation:
We can use to formula 
. Here, N(A) is the final amount. N0 is the initial amount. t is the time elapsed, and 
is the half life. Plugging in, we get the answer above.
Explanation:
The reactants are Aluminium and Copper chloride.
The products are Copper and Aluminium chloride.
Covalent Bond Name :N6Cl10
Explanation:
- Covalent compounds are named by using numerical prefixes to identify the number of atoms in the molecule. For example Carbon Dioxide CO2 and Carbon Monoxide CO . ... Drop the double vowel for the prefix and the element of the second element in the compound.
- The three types as mentioned in the other answers are polar covalent, nonpolar covalent, and coordinate covalent. The first, polar covalent, is formed between two nonmetals that have a difference in electronegativity. They share their electron density unevenly.
- Examples of Covalent Bond: Water. An example is water. Water consists of a covalent bond containing hydrogen and oxygen bonding together to make H2O. ...Diamonds. A diamond is an example of Giant Covalent bond of carbon. A diamond has a giant molecular structure. ...Vulcanized rubber. Another example is vulcanized rubber.
- Covalent bonds are especially important since most carbon molecules interact primarily through covalent bonding. Covalent bonding allows molecules to share electrons with other molecules, creating long chains of compounds and allowing more complexity in life.
I think it’s c I could be wrong
