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3 years ago

What is the volume of 23.4 grams of nitrogen gas at 750 mmHg and 28 degrees C

Chemistry

1 answer:

ratelena [41]3 years ago

6 0

Answer:

V = 20.97 L

Explanation:

Given data:

Mass of nitrogen = 23.4 g

Pressure of gas = 750 mmHg (750/760 = 0.99 atm)

Temperature of gas = 28°C (28+273= 301K)

Volume of gas = ?

Solution:

First of all we will calculate the number of moles of gas.

Number of moles = mass / molar mass

Number of moles = 23.4 g/ 28 g/mol

Number of moles = 0.84 mol

Now we will calculate the volume:

PV = nRT

V = nRT/P

R = general gas constant = 0.0821 atm.L/mol.K

V = 0.84 mol× 0.0821 atm.L/mol.K× 301 K / 0.99 atm

V = 20.76 L/0.99

V = 20.97 L

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Answer: Option (C) is the correct answer.

Explanation:

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cupoosta [38]

Answer:

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Explanation:

So this problem refers to Charles's law. You would use this formula..

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For your problem, it would look like this...

$\frac{10L}{1500k} = \frac{V_{F} }{750k}$

You would cross multiply and your answer would be 5L.

To reassure yourself that the answer is correct, Charles law states that the Volume and the Temperature are directly proportional. Meaning if your temperature is decreasing, your volume <u>has</u> to decrease.

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