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Vesnalui [34]
3 years ago
11

Cortisone consists of molecules, each of which contains 21 atoms of carbon (plus other atoms). the mass percentage of carbon in

cortisone is 69.98%. what is the molar mass of cortisone?
Chemistry
1 answer:
GalinKa [24]3 years ago
4 0

Now to solve this problem, we are given the number of atoms therefore we must first convert this into number of moles. We can do this by using the Avogadro’s number. Calculating for number of moles of Carbon:

number of moles Carbon = 21 atoms of carbon (1 mole / 6.022 x 10^23 atoms C)

number of moles Carbon = 3.49 x 10^-23 mol C

 

Converting this to mass by multiplying the molar mass of C:

mass Carbon = 3.49 x 10^-23 mol C (12 g / mol)

mass Carbon = 4.18 x 10^-22 g

 

Therefore the mass of one molecule of Cortisone is:

mass of 1 molecule Cortisone = 4.18 x 10^-22 g / 0.6998

mass of 1 molecule Cortisone = 5.98 x 10^-22 g per molecule

 

Converting this to mass per 1 mol of Cortisone, by using again the Avogadro’s number:

mass of 1 mol Cortisone = (5.98 x 10^-22 g / molecule) (<span>6.022 x 10^23  molecules / mol)</span>

mass of 1 mol Cortisone = 360.10 g / mol = molar mass of cortisone

 

Answer:

360.10 g / mol

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stich3 [128]

Answer:

Fe + CuCl2 = FeCl2 + Cu

Explanation:

This is already balanced.

5 0
3 years ago
What does stoichiometry use to relate moles of one molecule to moles of
Shkiper50 [21]
It is A I took it befor hope this helps:)
6 0
2 years ago
Alveoli are tiny sacs of air in the lungs. Their average diameter is 4.50 × 10−5 m. Calculate the uncertainty in the velocity of
Arisa [49]

<u>Answer:</u> The uncertainty in the velocity of oxygen molecule is 4.424\times 10^{-5}m/s

<u>Explanation:</u>

The diameter of the molecule will be equal to the uncertainty in position.

The equation representing Heisenberg's uncertainty principle follows:

\Delta x.\Delta p=\frac{h}{2\pi}

where,

\Delta x = uncertainty in position = d = 4.50\times 10^{-5}m

\Delta p = uncertainty in momentum  = m\Delta v

m = mass of oxygen molecule = 5.30\times 10^{-26}kg

h = Planck's constant = 6.627\times 10^{-34}kgm^2/s^2

Putting values in above equation, we get:

4.50\times 10^{-5}m\times 5.30\times 10^{-26}kg\times \Delta v=\frac{6.627\times 10^{-34}kgm^2/s}{2\times 3.14}\\\\\Delta v=\frac{6.627\times 10^{-34}kgm^2/s^2}{2\times 3.14\times 4.50\times 10^{-5}m\times 5.30\times 10^{-26}kg}=4.424\times 10^{-5}m/s

Hence, the uncertainty in the velocity of oxygen molecule is 4.424\times 10^{-5}m/s

8 0
3 years ago
A 20.0 g piece of aluminum at 5.00 C is dropped into 20.2 g of water at 90.00 C. The final temperature is 75.00 C. Use the First
bekas [8.4K]

Answer:

The specific heat of aluminium is 0.906 J/g°C

Explanation:

Step 1: data given

Mass of aluminium = 20.0 grams

Temperature = 5.00 °C

Mass of water = 20.2 grams

Temperature of water = 90.00 °C

The final temperature = 75.00 °C

Specific heat of water = 4.184 J/g°C

Step 2: calculate the specific heat of aluminium

heat won = heat lost

Qaluminium = -Qwater

Q = m*c* ΔT

m(aluminium * c(aluminium) *ΔT(aluminium = -m(water) * c(water) *ΔT(water)

⇒with m(aluminium) = mass of aluminium = 20.0 grams

⇒with c(aluminium) = the specific heat of aluminium = TO BE DETERMINED

⇒with ΔT(aluminium) = the change of temperature = T2 - T1 = 75.00 °C - 5.00 °C = 70.00 °C

⇒with m(water) = the mass of water = 20.2 grams

⇒with c(water) = the specific heat of water = 4.184 J/g°C

⇒with ΔT(water) = T2 - T1 = 75.00°C - 90.00 °C = -15.00 °C

20.0 * c(aluminium) * 70.00 = -20.2 * 4.184 * -15.00

c(aluminium) = 0.906 J/g°C

The specific heat of aluminium is 0.906 J/g°C

7 0
3 years ago
Explain how carbon’s bonding ability makes it unique.
STatiana [176]

\huge\fcolorbox{red}{pink}{Answer ♥}

The carbon atom is unique among elements in its tendency to form extensive networks of covalent bonds not only with other elements but also with itself. ... Moreover, of all the elements in the second row, carbon has the maximum number of outer shell electrons (four) capable of forming covalent bonds.

Hope it helps uh ✌️✌️✌️

Gud mrng

7 0
3 years ago
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