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max2010maxim [7]
3 years ago
9

What is the volume of 11.2 g of O2 at 7.78 atm and 415 K?

Chemistry
1 answer:
irina1246 [14]3 years ago
3 0

Answer:

1.53 L

Explanation:

Step 1: Given data

  • Mass of oxygen (m): 11.2 g
  • Pressure (P): 7.78 atm
  • Temperature (T): 415 K
  • Ideal gas constant (R): 0.0821 atm.L/mol.K

Step 2: Calculate the moles (n) corresponding to 11.2 g of oxygen

The molar mass of oxygen is 32.00 g/mol.

11.2 g × (1 mol/32.00 g) = 0.350 mol

Step 3: Calculate the volume of oxygen

We will use the ideal gas equation.

P × V = n × R × T

V = n × R × T / P

V = 0.350 mol × (0.0821 atm.L/mol.K) × 415 K / 7.78 atm

V = 1.53 L

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Calculate the number of grams in 4.56 x 1026 atoms of sodium phosphate. Be sure to balance the charges of sodium phosphate. Help
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Answer:

124225.91 g of Na₃PO₄

Explanation:

From the question given above, the following data were obtained:

Number of atoms of Na₃PO₄ = 4.56×10²⁶ atoms

Mass of Na₃PO₄ =?

From Avogadro's hypothesis,

6.02×10²³ atoms = 1 mole of Na₃PO₄

Next, we shall determine the mass of 1 mole of Na₃PO₄. This can be obtained as follow:

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4.56×10²⁶ atoms = (4.56×10²⁶ × 164)/6.02×10²³

4.56×10²⁶ atoms = 124225.91 g of Na₃PO₄

Therefore, 124225.91 g of Na₃PO₄ contains 4.56×10²⁶ atoms

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