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AveGali [126]
3 years ago
15

The density of a saline (salt) solution is 1.27 g/mL. What is the mass of 326 milliliters of the solution?

Chemistry
2 answers:
zlopas [31]3 years ago
7 0

Answer:

thx for the points

Explanation:

jeyben [28]3 years ago
4 0

Answer:

ghj

Explanation:

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Which subatomic particles affect the mass of an atom
klasskru [66]

Answer:

protons and neutrons

Explanation:

those particles account for 99.99% of mass

6 0
3 years ago
10. Which one of the following statements about sulfuric acid is correct? A. Sulfuric acid has little effect on metals.
Orlov [11]
C. Sulfuric acid is a strong oxidizing agent.
7 0
3 years ago
A 0.4272 g sample of an element contains 2.241 x 10 ^21 atoms . what is the symbol of the element?
grin007 [14]

Answer:

Likely \rm In (indium.)

Explanation:

Number of atoms: N = 2.241 \times 10^{21}.

Dividing, N, the number of atoms by the Avogadro constant, N_A \approx 6.023 \times 10^{23} \; \rm mol^{-1}, would give the number of moles of atoms in this sample:

\begin{aligned} n &= \frac{N}{N_{A}} \\ &\approx \frac{2.241 \times 10^{21}}{6.023 \times 10^{23}\; \rm mol^{-1}} \approx 3.72 \times 10^{-3}\; \rm mol \end{aligned}.

The mass of that many atom is m = 0.4272\; \rm g. Estimate the average mass of one mole of atoms in this sample:

\begin{aligned}M &= \frac{m}{n} \\ &\approx \frac{0.4272\; \rm g}{3.72 \times 10^{-3}\; \rm mol} \approx 114.82\; \rm g \cdot mol^{-1}\end{aligned}.

The average mass of one mole of atoms of an element (114.82\; \rm g \cdot mol^{-1} in this example) is numerically equal to the average atomic mass of that element. Refer to a modern periodic table and look for the element with average atomic mass 114.82. Indium, \rm In, is the closest match.

5 0
3 years ago
Protactinium has 516 years of half life how many decays will it go through to become 1/64th of the substance? ,
Ulleksa [173]

Answer:

  • 6 decays

Explanation:

Each half life period reduced the amount of substance by half

  • 64 = 2⁶
  • 1/64 = (1/2)⁶

So 6 of half life cycles or decays will go.

6 0
3 years ago
What would be the oxidation number of the atoms in these compounds?
sashaice [31]

Answer:

Oxidation state] is defined as the charge an atom might be imagined to have when electrons are counted according to an agreed-upon set of rules:

The oxidation state of a free element (uncombined element) is zero for a simple (monoatomic) ion, the oxidation state is equal to the net charge on the ion.

Hydrogen has an oxidation state of 1 and oxygen has an oxidation state of −2 when they are present in most compounds. (Exceptions to this are that hydrogen has an oxidation state of −1 in hydrides of active metals, e.g. LiH, and oxygen has an oxidation state of −1 in peroxides, e.g. H2O2 the algebraic sum of oxidation states of all atoms in a neutral molecule must be zero, while in ions the algebraic sum of the oxidation states of the constituent atoms must be equal to the charge on the ion.

The same is written in my textbook. But how am I supposed to find the ox. number of an atom, which is in compound like K2UO4?

8 0
3 years ago
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