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3 years ago

True or False Hypoxia results from higher oxygen levels.

Chemistry

2 answers:

OverLord2011 [107]3 years ago

8 0

Answer:

True

Explanation:

Atmospheric pressure reduces the amount of oxygen in the air, therefore leading to Hypoxia. Higher altitues contribute.

shtirl [24]3 years ago

5 0

The answer to this would be true

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0. 102 g of an unknown compound dissolved in 100. Ml of water has an osmotic pressure of 28. 1 mmhg at 20°c. Calculate the molar

Daniel [21]

The molar mass of the compound is 68 g/mol.

<h3>What is the molar mass?</h3>

The Osmotic pressure can be obtained from the relationship;

π= iCRT

π= osmotic pressure = 28.1 mmHg or 0.037 atm

i = Vant Hoff factor = 1

C = concentration = ?

R = gas constant = 0.082 atmLK-1Mol

T = temperature = 20°c + 273 = 293 K

C = π/iRT

C = 0.037/1 * 0.082 * 293

C = 0.0015 M

Now;

Number of moles = C/V = 0.0015/100 * 10^-3

= 0.015 moles

Number of moles = mass/molar mass

Molar mass = mass/Number of moles = 0. 102 g/ 0.015 moles = 68 g/mol

Learn more about molar mass:brainly.com/question/22997914

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2 years ago

The reason that Noble Gases do not react is because

sveticcg [70]

Answer:

Noble gases are odorless, colorless, nonflammable, and monotonic gases that have low chemical reactivity. The full valence electron shells of these atoms make noble gases extremely stable and unlikely to form chemical bonds because they have little tendency to gain or lose electrons.

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3 years ago

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2.<br> A chemical property is a change in

liberstina [14]

Answer:

the chemical composition of a substance.

Explanation:

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3 years ago

In your OWN words...HOW is Hydropower produced?

Lapatulllka [165]

Well by rushing water or moving water

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3 years ago

What is the mass in grams of oxygen gas that is required to produce 32.1 grams of maleic acid anhydride?

klemol [59]

Considering the reaction stoichiometry, the mass of oxygen gas that is required to produce 32.1 grams of maleic acid anhydride is 47.17 grams.

The balanced reaction is:

2 C₆H₆(l) + 9 O₂(g)→ 2 C₄H₂O₃(s) + 4 CO₂(g) + 4 H₂O(g)

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

C₆H₆: 2 moles
O₂: 9 moles
C₄H₂O₃: 2 moles
CO₂: 4 moles
H₂O: 4 moles

The molar mass of each compound is:

C₆H₆: 78 g/mole
O₂: 32 g/mole
C₄H₂O₃: 98 g/mole
CO₂: 44 g/mole
H₂O: 18 g/mole

By reaction stoichiometry, the following amounts of mass of each compound participate in the reaction:

C₆H₆: 2 moles× 78 g/mole= 156 grams
O₂: 9 moles× 32 g/mole= 288 grams
C₄H₂O₃: 2 moles× 98 g/mole= 196 grams
CO₂: 4 moles× 44 g/mole= 176 grams
H₂O: 4 moles× 18 g/mole= 72 grams

Then you can apply the following rule of three: If by stoichiometries 196 grams of C₄H₂O₃ are produced by 288 grams of O₂, 32.1 grams of C₄H₂O₃ are produced from how much mass of O₂?

$mass of O_{2} =\frac{32.1 grams of C_{4} H_{2} O_{3} x288 grams of O_{2}}{196grams of C_{4} H_{2} O_{3}}$

<u><em>mass of O₂= 47.17 grams</em></u>

Finally, the mass of oxygen gas that is required to produce 32.1 grams of maleic acid anhydride is 47.17 grams.

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3 years ago