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Dominik [7]
2 years ago
7

a 5.00 L sample of helium expands to 12.0 L at which point the pressure is measured to be 0.720atm. what was the original pressu

re of the gas
Chemistry
1 answer:
stepan [7]2 years ago
5 0

Answer:

The answer to your question is  Pressure 1 = 1.73 atm

Explanation:

Data

Volume 1 = 5 l

Pressure 1 = ?

Volume 2 = 12 l

Pressure 2 = 0.72 atm

Process

To solve this problem use Boyle's law to solve this problem

                 Pressure 1 x Volume 1 = Pressure 2 x Volume 2

-Solve for Pressure 1

                 Pressure 1 = Pressure 2 x Volume 2 / Volume 1

-Substitutiion

                 Pressure 1 = 0.72 x 12 / 5

-Simplification

                Pressure 1 = 8.64/5

-Result

                 Pressure 1 = 1.73 atm

You might be interested in
The two naturally occurring isotopes of antimony, 121Sb (57.21 percent) and 123Sb (42.79 percent), have masses of 120.904 and 12
Alex

Answer:

The correct answer is option c.

Explanation:

Formula used to determine an average atomic mass :

\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i

Mass of isotope Sb-121 = 120.904 amu

Fractional abundance of Sb-121 = 57.21% = 0.5721

Mass of isotope Sb-123 = 122.904 amu

Fractional abundance of Sb-123 = 42.79% = 0.4279

Average atomic mass of Sb:

120.904 amu\times 0.5721+ 122.904 amu\times 0.4279=121.7598 amu \approx 121.76 amu

7 0
2 years ago
What is the difference between a 1s orbital and a 2s orbital is that
iVinArrow [24]

Answer:

The main difference is their energy level, 2s orbital is higher than 1s orbital.

4 0
3 years ago
A mixture of carbon dioxide and helium gases is maintained in a 7.91 L flask at a pressure of 1.42 atm and a temperature of 33 °
Crank

Answer:

The gas mixture contains 1.038 grams of helium

Explanation:

<u>Step 1:</u> Data given

Volume of the flask = 7.91 L

Total Pressure = 1.42 atm

Temperature = 33 °C

Mass of CO2 = 8.25 grams

Molar mass of CO2 = 44.01 g/mol

Molar mass of He = 4 g/mol

<u>Step 2</u>: Calculate total number moles of gas

p*V = n*R*T

⇒ p = the pressure = 1.42 atm

⇒ V = the volume = 7.91 L

⇒ n= the number of moles = TO BE DETERMINED

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

⇒ T = the temperature = 33 °C = 306 Kelvin

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

n = (1.42*7.91)/(0.08206 * 306)

n = 0.447 moles

<u>Step 3</u>: Calculate moles of CO2

Moles CO2 = mass CO2 / Molar mass CO2

Moles CO2 = 8.25 grams / 44.01 g/mol

Moles CO2 = 0.1875 moles

<u>Step 4:</u> Calculate moles of Helium

Moles Helium = total moles of gas - moles of CO2

Moles Helium = 0.447 - 0.1875 = 0.2595 moles of helium

<u>Step 5: </u> Calculate mass of helium

Mass of helium = moles of helium * molar mass of helium

Mass of helium = 0.2595 moles * 4 g/mol

Mass of helium = 1.038 grams

The gas mixture contains 1.038 grams of helium

8 0
2 years ago
Which intermolecular forces increase rapidly with increasing molecular size?
blondinia [14]
LONDON DISPERSION FORCES
8 0
3 years ago
What mass of natural gas (ch4) must you burn to emit 272 kj of heat?
balandron [24]
CH4 + 2 O2 ---> CO2 + 2 H2O Q = 891,6 kJ / mol CH4

1 mol CH4 = 16 g

16 g ---- 891,6 kJ
x g ----- 272 kJ

x = 272 kJ × 16 g / 891,6 kJ = 4,88 g

You must burn 4,88 g of CH4.

:-) ;-)
7 0
2 years ago
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