Answer:
The heat required to vaporize 102.3 grams of H₂O(l) is 231198 J.
Explanation:
The heat required to vaporize 102.3 g of H₂O(l) can be calculated as follows:
Where:
q: is the heat
ΔHv: is the heat of vaporization of water = 2260 J/g
m: is the mass = 102.3
Therefore, the heat required to vaporize 102.3 grams of H₂O(l) is 231198 J.
I hope it helps you!
Answer:
34.611g
Explanation:
mass of metal = ?
density of metal = 1.39/cm³
volume = 24.9 cm³
density = mass/volume
mass = density × volume
= 1.39g/cm³ × 24.9 cm³
= 34.611g
B. Decomposition.
<span>The electrodes used must not react with the elements thus formed; platinum is favorite for these.</span>
Just look at the name, it tells you the longest C chain. Ending with hexane means that the longest carbon chain is 6 C's long.
Explanation:
when electronegativity difference is from 0.0 to 0.4 then bond formed between the two atoms is non-polar covalent in nature.
When electronegativity difference is greater than 0.4 and less than 1.8 then bond between the two atoms is a polar covalent bond.
When electronegativity difference is 1.8 or greater than the bond formed is ionic in nature.
According to the given fill ups, the reaction equation is as follows.
This means the new products are formed due to the change in chemical composition of the reactants.
- Hence, the equation shows a chemical reaction - the breaking and forming of chemical bonds that leads to a change in the composition of matter.
- And, in the given equation is a product.
- In the equation, is reactant.
- In , the type of bond that holds the two oxygen atoms together is a non-polar covalent bond.
- In , the type of bond that holds one of the hydrogen atoms to the oxygen atom is a polar covalent bond.
- The number of oxygen atoms on the left side of the equation is equal to the number of oxygen atoms on the right side.