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3 years ago

calculate the grams of oxygen gas present in a 2.50 L sample kept at 1.66 atm pressure and a temperature of 10.0 C

Chemistry

2 answers:

Ahat [919]3 years ago

8 0

Answer:

5.72 grams of O₂ are present in the sample

Explanation:

Let's calculate the moles of O₂ by the Ideal Gases Law.

P . V = n . R . T

1.66 atm . 2.50L = n . 0.082 . 283K

(1.66 atm . 2.50L) / 0.082 . 283K = n

0.179 mol = n

Molar mass O₂ = 32 g/m

Mol . molar mass = mass → 0.179 m . 32g/m = 5.72 g

Aloiza [94]3 years ago

7 0

Answer:

The mass of oxygen gas is 5.72 grams

Explanation:

Step 1: Data given

Volume of oxygen gas (O2) = 2.50L

Pressure of O2 gas = 1.66 atm

Temperature = 10.0 °C = 283 Kelvin

Step 2: Calculate moles of O2 gas

p*V = n*R*T

n = (p*V)/(R*T)

⇒ with n = the moles of O2 gas = TO BE DETERMINED

⇒ with p = the pressure of the O2 gas =1.66 atm

⇒ with V = the volume of the gas = 2.50 L

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

⇒ with T= the temperature = 10.0°C = 283 K

n = (1.66 * 2.50)/(0.08206*283)

n = 0.1787 moles O2

Step 3: Calculate mass of O2 grams

Mass O2 = moles O2 = Molar mass O2

Mass O2 = 0.1787 moles * 32.0 g/mol

Mass O2 = 5.72 grams

The mass of oxygen gas is 5.72 grams

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Read 2 more answers

A radioactive isotope of potassium (k) has a half-life of 20 minutes. if a 43 gram sample of this isotope is allowed to decay fo

Ksenya-84 [330]

Hello!

The half-life is the time of half-disintegration, it is the time in which half of the atoms of an isotope disintegrate.

We have the following data:

mo (initial mass) = 43 g

m (final mass after time T) = ? (in g)

x (number of periods elapsed) = ?

P (Half-life) = 20 minutes

T (Elapsed time for sample reduction) = 80 minutes

Let's find the number of periods elapsed (x), let us see:

$T = x*P$

$80 = x*20$

$80 = 20\:x$

$20\:x = 80$

$x = \dfrac{80}{20}$

$\boxed{x = 4}$

Now, let's find the final mass (m) of this isotope after the elapsed time, let's see:

$m = \dfrac{m_o}{2^x}$

$m = \dfrac{43}{2^{4}}$

$m = \dfrac{43}{16}$

$\boxed{\boxed{m = 2.6875\:g}}\end{array}}\qquad\checkmark$

I Hope this helps, greetings ... DexteR! =)

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4 years ago