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Vitek1552 [10]
3 years ago
5

Iodine chloride, ICl, can be made by the following reaction between iodine, I2, potassium iodate, KIO3, and hydrochloric acid.

Chemistry
2 answers:
Vadim26 [7]3 years ago
6 0
The balanced chemical reaction is:

<span>2 I2 + KIO3 + 6 HCl ---------> 5 ICl + KCl + 3 H2O 
</span>
We are given the amount of the product to be produced from the reaction. This will be the starting point of our calculations.

28.6 g ICl (1 mol / 162.35 g ICl ) ( 2 mol I2 / 5 mol ICl ) ( 253.81 g I2 / 1 mol I2 ) = 17.88 g I2
svet-max [94.6K]3 years ago
5 0

Answer:

You need 17.87 grams to prepare 28.6 grams of ICl

Explanation:

In first place you should verify that the following chemical equation is balanced:

2 I₂ + KIO₃ + 6 HCl ⇒ 5 ICl + KCl + 3H₂O

For that, you must first look at the subscripts next to each atom to find the number of atoms the molecule has. For example, KIO₃ have 1 atom of K, 1 atom of I and 3 atoms of O.

Then you must pay attention to the coefficient in front of each molecule, which tells us the amount of moles of that molecule that react or form.   For example, before I₂ there is a coefficient 2. This means that 2 moles of I₂ react. Then, to calculate the amount that react or are formed of each element, this coefficient is multiplied by the subindice of that element in each molecule. If the element appears in more than one molecule that reacts, the amounts are added. The same calculation is made with the products. So there are:

In reagents:

  • I: 5 atoms (coefficient 2 multiplied by subscript 2 of I₂ + coefficient 1 multiplied by subscript 1 of KIO₃)
  • K: 1 atom (coefficient 1 multiplied by subscript 1 of KIO₃)
  • O: 3 atoms (coefficient 1 multiplied by subscript 1 of KIO₃)
  • H: 6 atoms (coefficient 6 multiplied by subscript 1 of HCl)
  • Cl: 6 atoms (coefficient 6 multiplied by subscript 1 of HCl)

In products:

  • I: 5 atoms (coefficient 5 multiplied by subscript 1 of ICl)
  • K: 1 atom (coefficient 1 multiplied by subscript 1 of KCl)
  • O: 3 atoms (coefficient 3 multiplied by subscript 1 of H₂O)
  • H: 6 atoms (coefficient 3 multiplied by subscript 2 of H₂O)
  • Cl: 6 atoms (coefficient 5 multiplied by subscript 1 of ICl + coefficient 1 nultiplied by subscript 1 of KCl)

You can see that there is the same amount of each element in the reagents and in the products. So the chemical reaction is balanced.

Now you can calculate how many grams of iodine are needed to prepare 28.6 grams of ICl.  

The relationships between the different molecules according to the chemical reaction are in moles, so you must first know when moles are 28.6 grams of ICl.  For that you must know the molar mass of ICl, which is obtained with the molar mass of each element multiplied by the amount of that element in the molecule:

massmolarof ICl=126.9 \frac{grams}{mol} +35.45 \frac{grams}{mol} = 162.35 \frac{grams}{mol}

where 126.9 grams/mol is the mass of I and 35. 45 is the mass of Cl.

To determine how many moles are 28.6 grams you can do a simple rule of three:

If 162.35 grams are in 1 mole, how many moles are 28.6 grams?

molesofICl=\frac{28.6grams*1mole}{162.35 grams}

<em>molesofICl=0.176 moles</em>

Now you can use stoichiometric relationships, that is, the relationships that appear according to the chemical reaction, to calculate the amount of moles needed of I₂ to produce 0.176 moles of ICl. For that you do a simple rule of three:

If to produce 5 moles of ICl you need 2 moles of I₂  , how many moles of I₂ do you need to produce 0.176 moles of ICl?

molesofI2=\frac{0.176molesofICl*2molesofI2}{5moles of ICl}

<em>molesofI2=0.0704 moles</em>

So, you need 0.0704 moles of  I₂ to produce 0.176 moles of ICl.

Now,  knowing that the molar mass of I₂ is 253.8 grams (2*126.9 grams/mol), you can do a simple rule of three:

If 253.8 grams are in 1 mole, how many grams are in 0.0704 moles?

gramsofI2=\frac{0.0704 moles*253.8grams}{1mole}

<em>gramsofI2=17.87 grams</em>

<em>This means that you need 17.87 grams to prepare 28.6 grams of ICl</em>

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b) the weight-average molecular weight is 36,320 g/mol

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Explanation:

Given the data in the question;

Molecular                  Mean        Number      Weight      Number        Weight

weight                                                                             average         average

(g/mol)                    Mi(g/mol)         xi                wi          xiMi                  wiMi

8,000-16,000            12,000        0.07           0.03         840                360

16,000-24,000          20,000       0.15           0.09         3000              1800

24,000-32,000         28,000       0.26           0.21          7280              5880

32,000-40,000         36,000       0.27           0.27         9720               9720

40,000-48,000         44,000       0.18            0.28         7920              12320

48,000-56,000         52,000       0.07           0.12          3640              6240

∑                                                                                Mn=32,400     Mw=36,320

so;

a)  the number-average molecular weight

Mn = ∑Mixi

so from the table above; summation of Row Mixi

Mn = ∑Mixi = 32,400

Therefore, the number-average molecular weight is 32,400 g/mol

b) the weight-average molecular weight

Mw = ∑Miwi

so from the table above; summation of Row Miwi

Mw = ∑Miwi = 36,320

Therefore, the weight-average molecular weight is 36,320 g/mol

c) the degree of polymerization

the degree of polymerization of polypropylene can be determined using number-average molecular and repeat unit molecular weight.

now, for polypropylene { CH₂ = CH - CH₃ }

the repeat unit consist of 3 carbon atoms and 6 hydrogen atoms

given that;

Atomic weight of Carbon mC = 12.01 g/mol and

Atomic weight of  Hydrogen mH = 1.008 g/mol

now we find the repeat unit molecular weight of polypropylene

m = nCmC + nHmH

where n is the number of repeat of atoms

so we substitute

m = ( 3 × 12.01) + ( 6 × 1.008)

m = 36.03 + 6.048

m = 42.078 g/mol

now we calculate the degree of polymerization;

DP = Mn / m

so we substitute

DP = 32,400 / 42.078

DP = 769.9985 ≈ 770

Therefore,  the degree of polymerization is 770

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3.0 cm x 4.0 cm x 1.0 cm<br><br>[?]cm^3​
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Explanation:

<em>Hi</em><em> </em><em>there</em><em>!</em><em>!</em>

<em>you</em><em> </em><em>asked</em><em> </em><em>to</em><em> </em><em>multiply</em><em> </em><em>these</em><em> </em><em>all</em><em> </em><em>right</em><em>,</em>

<em>you</em><em> </em><em>can</em><em> </em><em>simply</em><em> </em><em>multiply</em><em> </em><em>it</em><em> </em><em>,</em>

<em>=</em><em>3</em><em>cm</em><em> </em><em>×</em><em> </em><em>4</em><em> </em><em>cm</em><em> </em><em>×</em><em> </em><em>1</em><em>cm</em>

<em>=</em><em> </em><em>1</em><em>2</em><em>cm</em><em>^</em><em>2</em><em>×</em><em>1</em><em>cm</em><em> </em><em> </em><em> </em><em> </em><em>(</em><em>4</em><em>×</em><em>3</em><em>=</em><em>1</em><em>2</em><em>)</em>

<em>=</em><em> </em><em>1</em><em>2</em><em>cm</em><em>^</em><em>3</em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em> </em><em>(</em><em>1</em><em>2</em><em>×</em><em>1</em><em>=</em><em>1</em><em>2</em><em>)</em>

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<em><u>Hope it helps</u></em><em><u>.</u></em><em><u>.</u></em>

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