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klio [65]
3 years ago
12

Calculate the number of moles of Cl atoms in 3.01×1024 formula units of magnesium chloride, MgCl2.

Chemistry
2 answers:
natta225 [31]3 years ago
8 0
Answer: 10 moles
To find how many moles, you need to divide the number of atoms with 6.02 * 10^23. Since every magnesium chloride has two chlorine atoms, you need to multiply it by 2. The calculation would be:  3.01×10^24  * 2 / 6.02 * 10^23= 10 moles
Elden [556K]3 years ago
6 0
The  number   of  moles  of  Cl  atom   is  calculated  by  use  of  avogadro  constant =  1  moles  =    6.02 x10^23
                 what  about    3.01  x10^24

(3.04  x10^24)/ ( 6.02  x   10^23)  =   5  moles

5  moles   is  for  CL  atom  what   about    CL2  in  MgCl2  =  2   x  5  =  10  moles
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Which of the following examples of erosion would occur most quickly?
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3 years ago
HELP ME PLEASE I NEED THE ANDEER NOW
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2 years ago
At a certain temperature the vapor pressure of pure benzene is measured to be . Suppose a solution is prepared by mixing of benz
Marianna [84]

Answer:

P(C₆H₆) = 0.2961 atm

Explanation:

I found an exercise pretty similar to this, so i'm gonna use the data of this exercise to show you how to do it, and then, replace your data in the procedure so you can have an accurate result:

<em>"At a certain temperature the vapor pressure of pure benzene (C6H6) is measured to be 0.63 atm. Suppose a solution is prepared by mixing 79.2 g of benzene and 115. g of heptane (C7H16) Calculate the partial pressure of benzene vapor above this solution. Round your answer to 2 significant digits. Note for advanced students: you may assume the solution is ideal".</em>

<em />

Now, according to the data, we want partial pressure of benzene, so we need to use Raoul's law which is:

P = Xₐ * P°    (1)

Where:

P: Partial pressure

Xₐ: molar fraction

P°: Vapour pressure

We only have the vapour pressure of benzene in the mixture. We need to determine the molar fraction first. To do this, we need the moles of each compound in the mixture.

To get the moles:   n = m / MM

To get the molar mass of benzene (C₆H₆) and heptane (C₇H₁₆), we need the atomic weights of Carbon and hydrogen, which are 12 g/mol and 1 g/mol:

MM(C₆H₆) = (12*6) + (6*1) = 78 g/mol

MM(C₇H₁₆) = (7*12) + (16*1) = 100 g/mol

Let's determine the moles of each compound:

moles (C₆H₆) = 79.2 / 78 = 1.02 moles

moles (C₇H₁₆) = 115 / 100 = 1.15 moles

moles in solution = 1.02 + 1.15 = 2.17 moles

To get the molar fractions, we use the following expression:

Xₐ = moles(C₆H₆) / moles in solution

Xₐ = 1.02 / 2.17 = 0.47

Finally, the partial pressure is:

P(C₆H₆) = 0.47 * 0.63

<h2>P(C₆H₆) = 0.2961 atm</h2>

Hope this helps

7 0
3 years ago
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