Molecule
Explanation:
The molecular formula HOH is an example of a molecule.
A molecule is the smallest particle of a substance (element or compound) capable of independent existence.
Molecules can be:
- Monoatomic with one atom e.g Neon, Argon
- Diatomic with two atoms e.g Nitrogen gas N₂
- Polyatomic e.g ozone O₃
The word molecule can also be used to refer to a covalent compound that has discrete or separate units.
The formula HOH or H₂O is a separate covalent that has an independent existence.
Learn more:
Molecules brainly.com/question/6071838
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Answer:
Beryllium-9 is the isotope of beryllium with relative atomic mass 9.
Answer:
0.78 M
Explanation:
First, we need to know which is the value of Kc of this reaction. In order to know this, we should take the innitial values of N2, O2 and NO and write the equilibrium constant expression according to the reaction. Doing this we have the following:
N2(g) + O2(g) <------> 2NO(g) Kc = ?
Writting Kc:
Kc = [NO]² / [N2] * [O2]
Replacing the given values we have then:
Kc = (0.6)² / (0.2)*(0.2)
Kc = 9
Now that we have the Kc, let's see what happens next.
We add more NO, until it's concentration is 0.9 M, this means that we are actually altering the reaction to get more reactants than product, which means that the equilibrium is being affected. If this is true, in the reaction when is re established the equilibrium, we'll see a loss in the concentration of NO and a gaining in concentrations of the reactants. This can be easily watched by doing an ICE chart:
N2(g) + O2(g) <------> 2NO(g)
I: 0.2 0.2 0.9
C: +x +x -2x
E: 0.2+x 0.2+x 0.9-2x
Replacing in the Kc expression we have:
Kc = [NO]² / [N2] * [O2]
9 = (0.9-2x)² / (0.2+x)*(0.2+x) ----> (this can be expressed as 0.2+x)²
Here, we solve for x:
9 = (0.9-2x)² / (0.2+x)²
√9 = (0.9-2x) / (0.2+x)
3(0.2+x) = 0.9-2x
0.6 + 3x = 0.9 - 2x
3x + 2x = 0.9 - 0.6
5x = 0.3
x = 0.06 M
This means that the final concentration of NO will be:
[NO] = 0.9 - (2*0.06)
[NO] = 0.78 M
Answer:
0.7644 moles of H₂O
Explanation:
The balance chemical equation is as follow;
2 H₂O₂ → 2 H₂O + O₂
To solve this problem we will first calculate the moles of H₂O₂ as,
Moles = Mass / M/Mass
Moles = 26.0 g / 34.01 g/mol
Moles = 0.7644 mol
Secondly,
According to equation,
2 moles of H₂O₂ produces = 2 moles of H₂O
Hence,
0.7644 mol of H₂O₂ will produce = X moles of H₂O
Solving for X,
X = 2 mol × 0.7644 mol / 2 mol
X = 0.7644 moles of H₂O
