Table of contents

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

General Chemistry

7. Gases

The Ideal Gas Law

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Multiple Choice

What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C, assuming ideal gas behavior?

1.02 atm

1.56 atm

2.10 atm

0.85 atm

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Verified step by step guidance

First, understand that the problem involves calculating the total pressure of a gas mixture using the ideal gas law. The ideal gas law is given by the equation:

P V = n R T

, where

P

is the pressure,

V

is the volume,

n

is the number of moles,

R

is the ideal gas constant, and

T

is the temperature in Kelvin.

Convert the temperature from Celsius to Kelvin. The conversion formula is:

T = T + 273.15

. For 20.0°C, the temperature in Kelvin is

20.0 + 273.15

Calculate the partial pressure of each gas using the ideal gas law. For hydrogen, use

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

with

n

as 0.127 mol,

R

as 0.0821 L·atm/mol·K,

T

as the converted temperature, and

V

as 6.00 L.

Similarly, calculate the partial pressure of nitrogen using the same formula, with

n

as 0.288 mol.

Add the partial pressures of hydrogen and nitrogen to find the total pressure in the flask. This is based on Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas.