Ideal Gas Law - AP Chemistry

1. Convert 25°C to Kelvin.

   298 K. Add 273.15 to convert Celsius to Kelvin.

2. What is an ideal gas?

   A hypothetical gas with perfectly elastic collisions. Gas with no intermolecular forces and negligible particle volume.

3. Identify the unit of pressure in the Ideal Gas Law.

   Atmospheres (atm). Standard unit of pressure in gas law calculations.

4. What is the relationship between temperature and kinetic energy?

   Directly proportional. Higher temperature means faster-moving gas molecules.

5. What does the variable $P$ represent in the Ideal Gas Law?

   Pressure. Force per unit area exerted by gas molecules on container walls.

6. Find $n$ if $P = 1$ atm, $V = 24.4$ L, $T = 298$ K.

   1 mol. Using $n = \frac{PV}{RT} = \frac{1 \times 24.4}{298 \times 0.0821}$.

7. Identify the proportionality in Charles's Law.

   Volume is directly proportional to temperature. At constant pressure, volume increases linearly with temperature.

8. State the formula for the Ideal Gas Law.

   $PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.

9. State the formula for the Ideal Gas Law.

   $PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.

10. Identify the proportionality in Boyle's Law.

    Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.

11. Identify the unit of the ideal gas constant $R$.

    L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.

12. What is the effect on pressure if moles double at constant $V$ and $T$?

    Pressure doubles. More gas particles create greater pressure at constant volume and temperature.

13. If $P = 2$ atm, $V = 5$ L, $T = 300$ K, find the moles of gas.

    0.406 mol. Using $n = \frac{PV}{RT} = \frac{2 \times 5}{0.0821 \times 300}$.

14. Identify the unit of temperature in the Ideal Gas Law.

    Kelvin (K). Absolute temperature scale required for gas law calculations.

15. State the combined gas law formula.

    $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$. Relates initial and final states when moles remain constant.

16. What does the variable $V$ stand for in the Ideal Gas Law?

    Volume. Space occupied by the gas, typically measured in liters.

17. State the formula for Boyle's Law.

    $P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.

18. Identify the proportionality in Boyle's Law.

    Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.

19. What happens to pressure if volume halves at constant $n$ and $T$?

    Pressure doubles. Inverse relationship from Boyle's Law at constant temperature.

20. State the formula for Avogadro's Law.

    $\frac{V_1}{n_1} = \frac{V_2}{n_2}$. Volume-moles relationship at constant pressure and temperature.

21. State the formula for Boyle's Law.

    $P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.

22. What does the variable $R$ represent in the Ideal Gas Law?

    Ideal gas constant. Universal constant relating gas properties, equal to 0.0821 L atm mol$^{-1}$ K$^{-1}$.

23. What is the effect on pressure if moles double at constant $V$ and $T$?

    Pressure doubles. More gas particles create greater pressure at constant volume and temperature.

24. What condition must be met for an ideal gas?

    Low pressure and high temperature. Minimal intermolecular forces and particle volume for ideal behavior.

25. State the formula for Boyle's Law.

    $P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.

26. State Gay-Lussac's Law formula.

    $\frac{P_1}{T_1} = \frac{P_2}{T_2}$. Pressure-temperature relationship at constant volume and moles.

27. Calculate the pressure when $n = 2$, $V = 10$ L, $T = 300$ K, $R = 0.0821$.

    4.92 atm. Using $P = \frac{nRT}{V} = \frac{2 \times 0.0821 \times 300}{10}$.

28. State the formula for Charles's Law.

    $\frac{V_1}{T_1} = \frac{V_2}{T_2}$. Volume-temperature relationship at constant pressure and moles.

29. Find the pressure when $V=10$ L, $T=300$ K, $n=1$ mol, $R=0.0821$

    2.46 atm. Using $P = \frac{nRT}{V} = \frac{1 \times 0.0821 \times 300}{10}$.

30. What does the variable $T$ represent in the Ideal Gas Law?

    Temperature in Kelvin. Absolute temperature scale where molecular motion ceases at 0 K.

31. What is the standard temperature in Kelvin?

    273 K. Absolute zero on the Kelvin scale, equivalent to 0°C.

32. What happens to volume if both $P$ and $T$ double?

    Volume remains the same. Both pressure and temperature changes cancel out in the ideal gas law.

33. What is the effect on volume if pressure triples at constant $T$?

    Volume decreases to one-third. Inverse relationship from Boyle's Law.

34. Calculate $T$ if $P = 3$ atm, $V = 5$ L, $n = 0.5$ mol, $R = 0.0821$.

    366 K. Using $T = \frac{PV}{nR} = \frac{3 \times 5}{0.5 \times 0.0821}$.

35. Identify the unit of volume in the Ideal Gas Law.

    Liters (L). Standard unit of volume in gas law calculations.

36. What does the variable $n$ represent in the Ideal Gas Law?

    Amount of substance in moles. Number of moles quantifies the amount of gas particles present.

37. Identify the unit of the ideal gas constant $R$.

    L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.

38. What is the effect on pressure if moles double at constant $V$ and $T$?

    Pressure doubles. More gas particles create greater pressure at constant volume and temperature.

39. What happens to volume if temperature doubles at constant $P$ and $n$?

    Volume doubles. Direct relationship from Charles's Law at constant pressure.

40. Determine the volume if $P = 1$ atm, $n = 1$ mol, $T = 273$ K, $R = 0.0821$.

    22.4 L. Molar volume of an ideal gas at STP (standard temperature and pressure).

41. State the value of the ideal gas constant $R$.

    0.0821 L atm mol$^{-1}$ K$^{-1}$. Standard value used in ideal gas calculations.

42. Convert 300 K to Celsius.

    27°C. Subtract 273.15 to convert Kelvin to Celsius.

43. Identify the law: Volume is constant as pressure and temperature change.

    Gay-Lussac's Law. Describes pressure-temperature relationship at constant volume.

44. State the formula for the Ideal Gas Law.

    $PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.

45. What does the variable $n$ represent in the Ideal Gas Law?

    Amount of substance in moles. Number of moles quantifies the amount of gas particles present.

46. What does the variable $n$ represent in the Ideal Gas Law?

    Amount of substance in moles. Number of moles quantifies the amount of gas particles present.

47. Identify the proportionality in Boyle's Law.

    Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.

48. Identify the proportionality in Avogadro's Law.

    Volume is directly proportional to moles. At constant pressure and temperature, volume scales with particle number.

49. Find the temperature if $P = 1$ atm, $V = 22.4$ L, $n = 1$ mol, $R = 0.0821$.

    273 K. Using $T = \frac{PV}{nR} = \frac{1 \times 22.4}{1 \times 0.0821}$.

50. If $P = 3$ atm and $T$ doubles, what is new $P$ at constant $V$?

    6 atm. Direct proportionality from Gay-Lussac's Law.

51. Identify the unit of the ideal gas constant $R$.

    L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.

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