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MrMuchimi
3 years ago
5

A student finds a container of gases in the laboratory classroom with a total pressure reading of 655 mmHg. The label on the con

tainer describes the contents as 5.00 g of carbon dioxide gas and 3.75 g of helium gas. Calculate the partial pressure of carbon dioxide in the container in mmHg.
Chemistry
1 answer:
Elena-2011 [213]3 years ago
6 0

Answer:

70.8 mmHg

Explanation:

To find partial pressure of carbon dioxide we first find the mole fraction of carbon dioxide

n (carbon dioxide) = 5/44.01 g/mol = 0.11361 mol

n (Helium) = 3.75 g/4 g/mol = 0.9375 mol

The partial pressure of carbon dioxide will be the mole fraction of carbon dioxide multiplied by the total pressure

Partial pressure = 0.11361g/(0.11361g + 0.9375 g)* 655 mmHg

                          = 70.8 mmHg

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a 1.25g sample of ore containing iron pyrite (FeS2) was pulverized and ignited in air, converting the FeS2 to Fe2O3 and SO2(g).
svp [43]

Answer:

28.9%

Explanation:

Let's consider the following balanced equation.

2 FeS₂ + 11/2 O₂ ⇒ Fe₂O₃ + 4 SO₂

We can establish the following relations:

  • The molar mass of Fe₂O₃ is 159.6 g/mol
  • 1 mole of Fe₂O₃ is produced per 2 moles of FeS₂
  • 1 mole of Fe is in 1 mole of FeS₂
  • The molar mass of Fe is 55.84 g/mol

The amount of Fe in the sample that produced 0.516 g of Fe₂O₃ is:

0.516gFe_{2}O_{3}.\frac{1molFe_{2}O_{3}}{159.6gFe_{2}O_{3}} .\frac{2molFeS_{2}}{1molFe_{2}O_{3}} .\frac{1molFe}{1molFeS_{2}} .\frac{55.84gFe}{1molFe} =0.361gFe

The percent of Fe in 1.25 g of the ore is:

\frac{0.361g}{1.25g} .100\%=28.9\%

4 0
3 years ago
How many atoms make up a diatomic molecule?
zalisa [80]
The prefix 'di' means two. Hence two atoms make up a diatomic molecule.
Hope this helps!
6 0
3 years ago
Why is the sky black in space
Shkiper50 [21]

Answer:Since there is virtually nothing in space to scatter or re-radiate the light to our eye, we see no part of the light and the sky appears to be black.

Explanation:

3 0
3 years ago
Question 7 of 15
Crazy boy [7]

Answer: 0.4 moles

Explanation:

Given that:

Volume of gas V = 11L

(since 1 liter = 1dm3

11L = 11dm3)

Temperature T = 25°C

Convert Celsius to Kelvin

(25°C + 273 = 298K)

Pressure P = 0.868 atm

Number of moles N = ?

Note that Molar gas constant R is a constant with a value of 0.00821 atm dm3 K-1 mol-1

Then, apply ideal gas equation

pV = nRT

0.868atm x 11dm3 = n x (0.00821 atm dm3 K-1 mol-1 x 298K)

9.548 atm dm3 = n x 24.47atm dm3mol-1

n = (9.548 atm dm3 / 24.47atm dm3 mol-1)

n = 0.4 moles

Thus, there are 0.4 moles of the gas.

3 0
2 years ago
Select the correct answer. Which property is typical of a covalent compound?
Vesnalui [34]

Answer:

it is b

Explanation:

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2 years ago
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