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LUCKY_DIMON [66]
3 years ago
15

If an isotope of an element has 33 neutrons and a mass number of 64, how many electrons must it have?

Chemistry
2 answers:
larisa [96]3 years ago
7 0
The mass number is the sum of the protons and neutrons
64 = #protons + #neutrons
Find the number of protons given the number of neutrons
64 = #protons + 33
#protons = 31
In a neutral element (such as this), the number of electrons equals the number of protons
#electrons = #protons
#electrons = 31
andrew-mc [135]3 years ago
6 0

Answer:

The isotope must have 31 electrons

Explanation:

  • Mass number = (number of neutrons)+(number of protons)
  • Here, mass number of element is 64 and number of neutrons is 33
  • So, number of protons i the element = (mass number)-(number of neutrons) = (64)-(33) = 31
  • Isotope of an element remain present in neutral form.
  • So, number of protons should be equal to number of electrons in that isotope. Because proton has +1 charge and electron has -1 charge
  • So, the isotope must have 31 electrons.
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The answer to question 2
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Answer:


12


Explanation:


You will need a chemical equation with masses and molar masses, so let’s gather all the information in one place.


M_{r}:                           258.21       18.02


                 KAl(SO₄)₂·xH₂O ⟶ KAl(SO₄)₂ + xH₂O


Mass/g:             4.74                                       2.16


Step 1. Calculate the mass of the KAl(SO₄)₂.


Mass = 4.74 g – 2.16 g = 2.58 g.


Step 2. Calculate the moles of each product.


\text{Moles of KAl(SO}_{4})_{2} = \text{2.58 g} \times \frac{\text{1 mol} }{\text{258.21 g}} = 9.992 \times 10^{-3} \text{ mol}

\text{Moles of H}_{2}\text{O} = \text{2.16 g} \times \frac{\text{1 mol} }{\text{18.02 g}} = \text{ 0.1200 mol}

Step 3. Calculate the molar ratio of the two products.


\frac{\text{Moles of KAl(SO}_{4})_{2}}{\text{Moles of H}_{2}\text{O}} = \frac{ 9.992 \times 10^{-3} \text{ mol}}{\text{ 0.1200 mol} } = \frac{1 }{12.01} \approx \frac{ 1}{ 12}

1 mol of KAl(SO₄)₂ combines with 12 mol H₂O, so x = 12.



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