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Natalija [7]
3 years ago
15

Osmium has a density of 22.6 g/cm3. What volume (in cm3) would be occupied by a 21.8 g sample of osmium? 1.04 2.03 × 103 493 0.9

65 2.03 × 10-3
Chemistry
1 answer:
vazorg [7]3 years ago
3 0

Answer:

volume =0.9645cm³

Explanation:

density refers to the ratio of mass to volume of a substance. It gives us a clue about how heavy an object is.

density = mass/volume

volume = mass/density

mass=21.8g

density=22.6g

volume =21.8/22.6

volume =0.9645cm³

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goldfiish [28.3K]

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If flame is not low then water as well as got spatter so it is important to use low flame so that   the water and filtrate will not spatter.


4 0
3 years ago
The chemical formula for table sugar is C 12 H 11 O 22 . What can you tell from this formula?
Paraphin [41]
The the last one, but isn't it c6h12o6?
8 0
3 years ago
How many moles of h+ are associated with the acid h2so3 during neutralization?
Katena32 [7]

H2SO3 or sulfurous acid is actually a strong acid. We know for a fact that strong acids completely dissociate into its component ions in a solution, that is:

 

<span>H2SO3 -->  2H+  +  SO3-</span>

 

<span>So from the equation above, there are 2 moles of H+</span>

8 0
3 years ago
What is the wavelength of radiation emitted when an electron goes from the n = 7 to the n = 4 level of the Bohr hydrogen atom? G
Phantasy [73]

Answer:

the wavelength of radiation emitted  is \mathbf{\lambda= 2169.62 \ nm}

Explanation:

The energy of the Bohr's hydrogen atom can be expressed with the formula:

\mathtt{E_n =- \dfrac{13.6\ ev}{n^2}}

For n = 7:

\mathtt{E_7 =- \dfrac{13.6\ ev}{7^2}}

\mathtt{E_7 =-0.27755 \ eV}

For n = 4

\mathtt{E_4=- \dfrac{13.6\ ev}{4^2}}

\mathtt{E_4 =- 0.85\ eV}

The  electron goes from the n = 7 to the n = 4, then :

\mathtt{E_7-E_4 = (-0.27755 - (-0.85) ) \ eV}

\mathtt{= 0.57245\ eV}

Wavelength of the radiation emitted:

\mathtt{\lambda= \dfrac{hc}{0.57245 \ eV}}

where;

hc  = 1242 eV.nm

\mathtt{\lambda= \dfrac{1242 \ eV.nm }{0.57245 \ eV}}

\mathbf{\lambda= 2169.62 \ nm}

4 0
3 years ago
Calculate the molarity of a solution<br> made by 1,5kg of K. CO₂ in 850 mL<br> of water.
anastassius [24]

Answer:

17.83M

Explanation:

Given parameters:

Mass of KCO₂ = 1.5kg

Volume of water  = 850mL

Unknown:

Molarity of solution  = ?

Solution:

Molarity is defined as the number of moles per unit volume. It is the number of moles of solute in a given volume of solution.

   Molarity  = \frac{number of moles }{volume}

Number of moles of solute  = \frac{mass of KCO_{2} }{molar mass}

  Molar mass of KCO₂  = 39 + 12 + 3(16) = 99g/mol

  Number of moles  = \frac{1500}{99}   = 15.15moles

   850mL : gives 0.85L

     

Molarity  = \frac{15.15}{0.85}   = 17.83M

8 0
3 years ago
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