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vesna_86 [32]
3 years ago
8

Given that P-31 is the only natural isotope of phosphorus, what is the mass of one P atom and the mass of Avogadro's number of P

atoms, respectively?
Chemistry
2 answers:
Citrus2011 [14]3 years ago
5 0

Answer:

Mass of Avogadro's number of P atoms = 31 g

Mass of 1 P atom = 5.15*10⁻²³ g

Explanation:

The two rules to consider are:

1) Mass of 1 mole of an element is equal to its molar mass in grams

2) 1 mole of any element contains Avogadro's number of atoms

i.e. 1 mole = 6.023*10^23 atoms(or molecules or particles)

For P-31

1 mole of P-31 = 31 grams

i.e. Mass of Avogadro's number of P atoms = 31 g

6.023*10^23 P atoms = 31 g

Therefore, mass of 1 P atom is:

= \frac{1\ P\ atom *31\ g}{6.023*10^{23}\ atoms}=5.15*10^{-23}\ g

Sonja [21]3 years ago
3 0
The mass of on P atom would be 31 divided by 6.02 * 10^23
The mass of Avogadro's number of P atoms would be 31, since the atomic weight of and element is the mass of exactly one mole of that element, and Avogadro's number is the number of atoms in one mole.
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In a mixture of 2 ideal gases, A and B, PA = 0.2PB, what is the mole fraction of A?
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Answer:

0.1667

Explanation:

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Dalton's law defines:

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A sample of nitrogen gas had a volume of 500. ml, a pressure in its closed container of 740 torr and a temperature 25 degrees c
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Question:
              <span>A sample of nitrogen gas had a volume of 500mL, a pressure in its closed container of 740 torr and a temperature of 25°c. what was the volume of gas when the temperature was changed to 50°c and the new pressure was 760 torr?

Answer:

Data Given:
                   V</span>₁  =  500 mL

                   P₁  =  740 torr

                   T₁  =  25 °C + 273  =  298 K

                   V₂  =  ?

                   P₂  =  760 torr

                   T₂  =  50 °C + 273  =  323 K

Solution:
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                      P₁ V₁ / T₁  =  P₂ V₂ / T₂

Solving for V₂,

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Putting Values,
  
                      V₂  =  (740 torr × 500 mL × 323 K) ÷ (298 K × 760 torr)

                      V₂  =  527.68 mL
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