Answer:
H₂O.
Explanation:
- It is clear from the balanced equation:
<em>CH₄ + 2H₂O → CO₂ + 4H₂.</em>
that 1.0 mole of CH₄ reacts with 2.0 moles of H₂O to produce 1.0 mole of CO₂ and 4.0 moles of H₂.
- To determine the limiting reactant, we should calculate the no. of moles of (20 g) CH₄ and (15 g) H₂O using the relation:
<em>n = mass/molar mass</em>
<em></em>
no. of moles of CH₄ = mass/molar mass = (20 g)/(16 g/mol) = 1.25 mol.
no. of moles of H₂O = mass/molar mass = (15 g)/(18 g/mol) = 0.833 mol.
- <em>from the balanced reaction, 1.0 mole of CH₄ reacts with 2.0 moles of H₂O.</em>
So, from the calculated no. of moles: 0.4167 mole of CH₄ reacts completely with 0.833 mole of H₂O and the remaining of CH₄ will be in excess.
<u><em>So, the limiting reactant is H₂O.</em></u>
Bromine and Iodine are both
totally soluble in mineral oil because these substances are all made up of
non-polar molecules. And because water is a polar molecule, Bromine and Iodine
is not soluble in it.
Non polar solvents contain
bonds that have similar electronegativity, an example of this is carbon and
hydrogen such as gasoline. Some other examples are pentane, hexane, benzene
and toluene.
<span> </span>
Waters boiling point is 100°C and 212°F
Answer:
Aluminium (Al): (3*2)+(5*2)=16
Sulphor (S): (3*1)=3
Oxygen (O): (4*3)+(3*1)=15
3.0e23 atoms Ne
"E" means 10^
Then we multiply it by a mole of Ne. By the definetion of a mole, it is always 6.022e23 atoms of an element.
So now, we do this:
3.0e23 atoms Ne x (1 mol Ne / 6.022e23 atoms Ne)
After that, we use molar mass. A mole of Neon is equal, in terms of grams, to its avg. atomic mass. This goes true for any element.
It ends up like this:
3.0e23 atoms Ne x (1 mol Ne / 6.022e23 atoms Ne) x (20.1797 g Ne / 1 mol Ne)
Now cancel out the "atoms Ne" and "1 mol Ne"
You end up with a grand total of...
*plugs everything into a calculator*
10.05298... g Ne.
We need to round to 2 sig. figs. (3.0) so now it's....
10 g Ne.
Note that this method can only be used for converting atoms of an element to mass in grams.
Source(s):
A periodic table for the atomic mass of neon.
A chemistry textboook
A chemistry class.
