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1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

11 Gases

The Ideal Gas Law

Introduction to Chemistry

11 Gases

The Ideal Gas Law

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Multiple Choice

How many grams of carbon dioxide, CO₂, are present in a 0.150 L flask recorded at 525 mmHg and 32 ºC?
a) 1.77 g
b) 0.93 g
c) 0.66 g
d) 0.18 g
e) 0.052 g

1.77 g

0.93 g

0.66 g

0.18 g

0.052 g

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Verified step by step guidance

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: T(K) = 32 + 273.15.

Convert the pressure from mmHg to atm using the conversion factor: 1 atm = 760 mmHg. Calculate P(atm) = 525 mmHg / 760 mmHg.

Use the ideal gas law equation, PV = nRT, to solve for the number of moles (n) of CO2. Rearrange the equation to n = PV / RT, where R is the ideal gas constant (0.0821 L·atm/mol·K).

Substitute the values for P, V, and T into the equation to calculate the number of moles of CO2: n = (P(atm) * 0.150 L) / (0.0821 L·atm/mol·K * T(K)).

Convert the moles of CO2 to grams using the molar mass of CO2 (44.01 g/mol): mass (g) = n * 44.01 g/mol.