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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

7. Gases

The Ideal Gas Law: Molar Mass

General Chemistry

7. Gases

The Ideal Gas Law: Molar Mass

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Multiple Choice

Nitrogen gas is produced in a reaction. If the temperature of the gas is 225.5 K, the pressure is 13.9 MPa, and the volume is 13.0 L, determine the mass of the nitrogen gas in kilograms using the Ideal Gas Law.

0.324 kg

0.243 kg

0.162 kg

0.081 kg

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Verified step by step guidance

Start by recalling the Ideal Gas Law, which is expressed as:

P V = n R T

, where

P

is pressure,

V

is volume,

n

is the number of moles,

R

is the ideal gas constant, and

T

is temperature.

Convert the pressure from MPa to Pa for consistency with the ideal gas constant units. Since 1 MPa = 1,000,000 Pa, multiply 13.9 MPa by 1,000,000 to get the pressure in Pa.

Use the Ideal Gas Law to solve for the number of moles

n

. Rearrange the equation to

n = \frac{P V}{R T}

. Substitute the values for

P

V

R

(8.314 J/mol·K), and

T

into the equation.

Calculate the number of moles

n

using the rearranged Ideal Gas Law equation.

Convert the number of moles to mass. Use the molar mass of nitrogen gas,

28.02

g/mol, to find the mass in grams. Then, convert the mass from grams to kilograms by dividing by 1,000.

0:51m

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