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vazorg [7]
3 years ago
12

How much pressure would 0.8 moles of a gas at 370K exert if it occupied 17.3L of space

Chemistry
2 answers:
dezoksy [38]3 years ago
7 0

Answer:

1.40 atm is the pressure for the gas

Explanation:

An easy problem to solve with the Ideal Gases Law:

P . V = n . R .T

T° = 370K

V = 17.3L

n = 0.8 mol

Let's replace data → P . 17.3L = 0.8mol . 0.082L.atm/mol.K . 370K

P = (0.8mol . 0.082L.atm/mol.K . 370K) / 17.3L = 1.40 atm

DerKrebs [107]3 years ago
3 0

Answer:

The pressure is 1.40 atm

Explanation:

Step 1: Data given

Number of moles = 0.8 moles

Temperature = 370 K

volume = 17.3 L

Step 2: Calculate the pressure

p*V = n*R*T

⇒ with p = the pressure = TO BE DETERMINED

⇒with V = the volume = 17.3 L

⇒with n = the number of moles of gas = 0.8 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 370 K

p = (n*R*T)/V

p = (0.8 * 0.08206 * 370) / 17.3 L

p = 1.40 atm

The pressure is 1.40 atm

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Answer:

The amount of heat required to raise the temperature of a 32g sample of water from 8°C to 22°C is 1,874.432 J

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

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In this case:

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Solving:

Q= 1,874.432 J

<u><em>The amount of heat required to raise the temperature of a 32g sample of water from 8°C to 22°C is 1,874.432 J</em></u>

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18.35 mL of an HCN solution were titrated with 35.4mL of a 0.268M NaOH solution to reach the equivalence point. What is the mola
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Answer:

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