Water found in animal and human cells is most often found in the liquid phase of matter, and oxygen is found in the gas plasma <span>phase of matter. </span>
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Answer:
Molarity of our solution= 0.46=0.5
Explanation:
When diluting a solution we can use the formula:
1
1
=
2
2
= M= Molarity of the solution
=V=volumes
On the left side, we'll put what we know/already have and on the right side of the formula we'll put down what we want to dilute it to.
Let's plug in what we already know.
(0.700M)(2L) = (M2)(3L)
Solve for M2 by dividing both sides by 3 so M2 will be by itself.
(0.700M)(2L)/(3L) = M2
M2= 0.46, we can round it up to 0.5
1 bulb b and c wouldn't shine if ac. if DC then yes. 2 a would shine and c wouldn't if DC if ac then yes
Answer:
half-life=T= 36.9 years
Explanation:
As we know that
N
(
t
)
=
N
(
0
)
⋅
0.5
^(t/
T
)
N
(
0
)
=the number of atoms you start with=20 gram
and N
(
t
)= the number of atoms left=0.625 grams
after a certain time=t=184.5 years
T=half life of a nuclide=?
Putting value in above equation we get
half-life=T= 36.9 years
.
Answer: 1. ![NH_3=82.4\%](https://tex.z-dn.net/?f=NH_3%3D82.4%5C%25)
2. ![CO(NH_2)_2=46.7\%](https://tex.z-dn.net/?f=CO%28NH_2%29_2%3D46.7%5C%25)
3. .
4.
has highest nitrogen content.
Explanation:
To calculate the mass percent of element in a given compound, we use the formula:
1.
![\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of} NH_3}=\frac{14}{17}\times 100=82.4\%](https://tex.z-dn.net/?f=%5Ctext%7BMass%20percent%20of%20nitrogen%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20nitrogen%7D%7D%7B%5Ctext%7BMass%20of%7D%20NH_3%7D%3D%5Cfrac%7B14%7D%7B17%7D%5Ctimes%20100%3D82.4%5C%25)
2.
![\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of} CO(NH_2)_2}=\frac{14\times 2}{12\times 1+16\times 1+2\times 14+4\times 1}\times 100=\frac{28}{60}\times 100=46.7\%](https://tex.z-dn.net/?f=%5Ctext%7BMass%20percent%20of%20nitrogen%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20nitrogen%7D%7D%7B%5Ctext%7BMass%20of%7D%20CO%28NH_2%29_2%7D%3D%5Cfrac%7B14%5Ctimes%202%7D%7B12%5Ctimes%201%2B16%5Ctimes%201%2B2%5Ctimes%2014%2B4%5Ctimes%201%7D%5Ctimes%20100%3D%5Cfrac%7B28%7D%7B60%7D%5Ctimes%20100%3D46.7%5C%25)
3.
![\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of} NH_4NO_3}=\frac{14\times 2}{14\times 2+16\times 3+4\times 1}\times 100=\frac{28}{80}\times 100=35\%](https://tex.z-dn.net/?f=%5Ctext%7BMass%20percent%20of%20nitrogen%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20nitrogen%7D%7D%7B%5Ctext%7BMass%20of%7D%20NH_4NO_3%7D%3D%5Cfrac%7B14%5Ctimes%202%7D%7B14%5Ctimes%202%2B16%5Ctimes%203%2B4%5Ctimes%201%7D%5Ctimes%20100%3D%5Cfrac%7B28%7D%7B80%7D%5Ctimes%20100%3D35%5C%25%20)
4.
![\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of}(NH_4)_2SO_4}=\frac{14\times 2}{14\times 2+16\times 4+32\times 1+8\times 1}\times 100=\frac{28}{132}\times 100=21.2\%](https://tex.z-dn.net/?f=%5Ctext%7BMass%20percent%20of%20nitrogen%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20nitrogen%7D%7D%7B%5Ctext%7BMass%20of%7D%28NH_4%29_2SO_4%7D%3D%5Cfrac%7B14%5Ctimes%202%7D%7B14%5Ctimes%202%2B16%5Ctimes%204%2B32%5Ctimes%201%2B8%5Ctimes%201%7D%5Ctimes%20100%3D%5Cfrac%7B28%7D%7B132%7D%5Ctimes%20100%3D21.2%5C%25)
Thus
has highest nitrogen content of 82.4%.