Chemistry : asked on cdraytonn
 14.01.2023

A diver planning to dive to a depth of 100 ft can choose to breathe air that is a mixture of oxygen, nitrogen, and helium. If the total pressure of the air in the tank is 3040 mm Hg , and the partial pressures of O2 and He are 304 mm Hg and 1520 mm Hg , respectively, what is the partial pressure of N2

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24.06.2023, solved by verified expert
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1216 mmHg = Partial pressure N₂

Explanation:

In a mixture of n gases, the partial pressure of each compound follows the equation:

Total pressure = Partial pressure n₁ + Partial pressure n₂ + Partial pressure n₃ + Partial pressure n₄ + Partial pressure n₅ + ... + Partial pressure nₙ

In a mixture of O₂, He and N₂, the total pressure = 3040mmHg is defined as:

3040 mmHg = Partial pressure O₂ + Partial pressure He + Partial pressure N₂

Replacing:

3040 mmHg = 304 mmHg + 1520 mmHg + Partial pressure N₂

3040 mmHg = 1824 mmHg + Partial pressure N₂

1216 mmHg = Partial pressure N₂

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Chemistry
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P Answered by PhD

1216 mmHg = Partial pressure N₂

Explanation:

In a mixture of n gases, the partial pressure of each compound follows the equation:

Total pressure = Partial pressure n₁ + Partial pressure n₂ + Partial pressure n₃ + Partial pressure n₄ + Partial pressure n₅ + ... + Partial pressure nₙ

In a mixture of O₂, He and N₂, the total pressure = 3040mmHg is defined as:

3040 mmHg = Partial pressure O₂ + Partial pressure He + Partial pressure N₂

Replacing:

3040 mmHg = 304 mmHg + 1520 mmHg + Partial pressure N₂

3040 mmHg = 1824 mmHg + Partial pressure N₂

1216 mmHg = Partial pressure N₂

Chemistry
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P Answered by PhD

Answer:

52.6 gram

Step-by-step explanation:

It is clear by the equation 2(27+3×35.5)= 267 gm of AlCl3 reacts with 6× 80 = 480 gm of Br2 . So 29.2 gm reacts = 480× 29.2/267= 52.6 gm

Chemistry
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P Answered by PhD

glycoproteins

Explanation:

A positive reaction for Molisch's test is given by almost all carbohydrates (exceptions include tetroses & trioses). It can be noted that even some glycoproteins and nucleic acids give positive results for this test (since they tend to undergo hydrolysis when exposed to strong mineral acids and form monosaccharides).

Chemistry
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P Answered by PhD

Answer:

Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:  

P×V = n×R×T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances.

Explanation:

In this case, you know:

P= 0.884 atm

V= ?

n= Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N 0.857 moles (where 28 g/mole is the molar mass of N₂, that is, the amount of mass that the substance contains in one mole.)

R=0.082Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N

T= 328 K

Replacing in the ideal gas law:

0.884 atm×V= 0.857 moles× 0.082Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N ×328 K

Solving:

Answer:Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N

V= 26.07 L

The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.

Chemistry
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P Answered by PhD
Answer: 25 g
Explanation: Given:
Original amount (N₀) = 100 g
Number of half-lives (n) = 11460/5730 = 2
Amount remaining (N) = ?
N = 1/2ⁿ × N₀
N = 1/2^2 × 100
N = 0.25 × 100
N = 25 g
Chemistry
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P Answered by PhD
Answer: 7.8125 g
Explanation: Given:
Original amount (N₀) = 500 g
Number of half-lives (n) = 9612/1602 = 6
Amount remaining (N) = ?
N = 1/2ⁿ × N₀
N = 1/2^6 × 500
N = 0.015625 × 500
N = 7.8125 g
Chemistry
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P Answered by PhD
Answer: The product formed is potassium chloride.
Explanation:
Precipitation reaction is defined as the chemical reaction in which an insoluble salt is formed when two solutions are mixed containing soluble substances. The insoluble salt settles down at the bottom of the reaction mixture.

The chemical equation for the reaction of potassium phosphate and magnesium chloride follows (look at the picture)

2 moles of aqueous solution of potassium phosphate reacts with 3 moles of aqueous solution of magnesium chloride to produce 1 mole of solid magnesium phosphate and 6 moles of aqueous solution of potassium chloride.
Answer: The product formed is potassium chloride.
Explanation:
Precipitation reaction is defined a
Chemistry
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P Answered by PhD
Answer: a. basic
b. basic
c. acidic
d. neutral

Explanation: Acids and bases can be classified in terms of hydrogen ions or hydroxide ions, or in terms of electron pairs. (look at the picture)
Let us note that from the pH scale, a pH of;
0 - 6.9 is acidic
7 is neutral
8 - 14 is basic

But pH= - log [H^+]
pOH = -log [OH^-]
Then;
pH + pOH = 14
Hence;
pH = 14 - pOH

a. [H+] = 6.0 x 10-10M
pH= 9.22 is basic
b. [OH-] = 30 × 10-2M
pH = 13.5 is basic
C. IH+1 = 20× 10-7M
pH = 0.56 is acidic
d. [OH-] = 1.0 x 10-7M
pH = 7 is neutral
Answer: a. basic
b. basic
c. acidic
d. neutral

Explanation: Acids and bases can be classified
Chemistry
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P Answered by PhD
Answer: 306 L
Explanation: Using the ideal gas law,
PV = nRT
where R = 0.08206 L•atm/(mol•°K), solving for n gives
n = PV/(RT)
n = (845 mmHg) (270 L) / ((0.08206 L•atm/(mol•°K)) (24 °C))

Convert the given temperature to °K and the given pressure to atm:
24 °C = (273.15 + 24) °K ≈ 297.2 °K
(845 mmHg) × (1/760 atm/mmHg) ≈ 1.11 atm

Then the balloon contains
n = (1.11 atm) (270 L) / ((0.08206 L•atm/(mol•°K)) (297.2 °K))
n ≈ 12.3 mol
of He.

Solve the same equation for V :
V = nRT/P

Convert the target temperature to °K:
-50 °C = (273.15 - 50) °K = 223.15 °K

Then the volume under the new set of conditions is
V = (12.3 mol) (0.08206 L•atm/(mol•°K)) (223.15 °K) / (0.735 atm)
V ≈ 306 L
Chemistry
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P Answered by PhD
Answer: -166.67 degrees Celsius.
Explanation: The equation of state of an ideal gas, also called the Mendeleev-Clapeyron equation, has the form: PV = nRT, where P is the density of the gas, V is the volume of the gas, n is the molar mass of the gas, T is the temperature of the gas, R is the universal gas constant = 8.314 J/(mol*K)
The gas temperature at a pressure of P = 978 mm. mercury column, molar mass n = 3.7 mol, and volume V = 25.12 liters is -166.67 degrees Celsius.

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