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dedylja [7]
3 years ago
8

Calculate the mole fraction of each component in a solution of 42 g CH3OH, 35 g of chloroform CHCl3, and 50 g C3H7OH

Chemistry
1 answer:
koban [17]3 years ago
4 0

Considering the definition of mole fraction, the mole fraction of each component in the solution is:

  • CH₃OH: 0.54
  • CHCl₃: 0.118
  • C₃H₇OH: 0.342

<h3>Mole fraction</h3>

The molar fraction is a way of measuring the concentration that expresses the proportion in which a substance is found with respect to the total moles of the solution.

<h3>Mole fraction of each component</h3>

In this case, in first place you should know that the molar mass of each component is:

  • CH₃OH: 32 \frac{g}{mole}
  • CHCl₃: 121.35 \frac{g}{mole}
  • C₃H₇OH: 60 \frac{g}{mole}

Now, the number of moles of each compound can be calculated as:

  • CH₃OH: \frac{42 g}{32\frac{g}{mole}}=  1.3125 moles
  • CHCl₃: \frac{35 g}{121.35\frac{g}{mole}}= 0.2884 moles
  • C₃H₇OH: \frac{50 g}{60\frac{g}{mole}}=  0.8333 moles

So, the total moles of the solution can be calculated as:

Total moles = 1.3125 moles + 0.2884 moles + 0.8333 moles

<u><em>Total moles = 2.4342 moles</em></u>

Finally, the more fraction of each component can be calculated as follow:

  • CH₃OH: \frac{1.3125 moles}{2.4342 moles}= 0.54
  • CHCl₃: \frac{0.2884 moles}{2.4342 moles}= 0.118
  • C₃H₇OH: \frac{0.8333 moles}{2.4342 moles}= 0.342

In summary, the mole fraction of each component in the solution is:

  • CH₃OH: 0.54
  • CHCl₃: 0.118
  • C₃H₇OH: 0.342

Learn more about mole fraction:

brainly.com/question/14434096

brainly.com/question/10095502

#SPJ1

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Answer: The volume of the gold is   75.68g/cm^3

The mass of gold is 19.3 g

The density of gold is 0.25g/cm^3

Explanation:

Density is defined as the mass contained per unit volume.

Density=\frac{mass}{Volume}

Given : Mass of gold = 19.3 grams

To calculate the volume of cube, we use the equation:

V=a^3

where,

V = volume of cube

a = edge of cube

Volume of gold = (4.23cm)^3=75.68cm^3

Putting values in above equation, we get:

Putting in the values we get:

Density=\frac{19.3g}{75.68cm^3}=0.25g/cm^3

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Which of the following factors would reduce the yield of a reaction?
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Answer:

B. The reactants form additional unexpected products.

Explanation:

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A compound with a molar mass of 100.0 g/lol has an elemental composition of 24.0% C, 3.0% H, 16.0% O and 57.0%F. What is the mol
ch4aika [34]

If I made no mistake in calculation, the given answer must be correct...(tried my best)



elements   :                        carbon     hydrogen    oxygen       Fluorine

 composition [C]                     24             3                16                57

M r                                          12             1                16                19

(divide C by Mr)                       2               3                 1                  3


(Divide by smallest value)       2                3                  1                  3

(smallest value = 1...so all value remained constant)

Empirical formula : C2H3OF3


if molar mas = 100 g per mole, then

first step calculate Mr. of empirical formula:  [= 100]


Them molecular formula = empirical formula

    
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4 years ago
What is the concentration, in millimolar, of a 1 mg/ml solution of NaCl (molecular weight = 58 Da)?
sineoko [7]

Explanation:

Relation between molarity and molar mass is as follows.

             Molarity = \frac{mass}{\text{molar mass}} \times \frac{1000}{V (in ml)}

It is given that mass is 1 mg/ml which is also equal to 10^{-3} g.

Molecular mass = 58 Da = 58 g/mol

Volume = 1 ml

Therefore, calculate molarity as follows.

         Molarity = \frac{mass}{\text{molar mass}} \times \frac{1000}{V (in ml)}

                       = \frac{10^{-3}g}{58 g/mol} \times \frac{1000}{1 ml}  

                       = 0.0172 molar

It is known that 1 molar equals 1000 millimolar.

So,               0.0172 molar = 0.0172 molar \times \frac{1000 millimolar}{1 molar}

                                          = 17.2 millimolar

Thus, we can conclude that the concentration of given solution is 17.2 millimolar.

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How to show the slope calculation of g (using proper units) and calculate the percent error of your experimental value?
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solution;

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= 0.25335

% error  = \frac{0.25335}{9.80665\times100}

= 2.583 %


8 0
3 years ago
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