Ideal Gas Law - AP Chemistry
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What does the variable $n$ represent in the Ideal Gas Law?
What does the variable $n$ represent in the Ideal Gas Law?
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Amount of substance in moles. Number of moles quantifies the amount of gas particles present.
Amount of substance in moles. Number of moles quantifies the amount of gas particles present.
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What is the effect on pressure if moles double at constant $V$ and $T$?
What is the effect on pressure if moles double at constant $V$ and $T$?
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Pressure doubles. More gas particles create greater pressure at constant volume and temperature.
Pressure doubles. More gas particles create greater pressure at constant volume and temperature.
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Identify the unit of the ideal gas constant $R$.
Identify the unit of the ideal gas constant $R$.
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L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.
L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.
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Identify the proportionality in Boyle's Law.
Identify the proportionality in Boyle's Law.
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Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.
Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.
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State the formula for Boyle's Law.
State the formula for Boyle's Law.
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$P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.
$P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.
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State the formula for the Ideal Gas Law.
State the formula for the Ideal Gas Law.
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$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.
$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.
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What does the variable $n$ represent in the Ideal Gas Law?
What does the variable $n$ represent in the Ideal Gas Law?
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Amount of substance in moles. Number of moles quantifies the amount of gas particles present.
Amount of substance in moles. Number of moles quantifies the amount of gas particles present.
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What is the effect on pressure if moles double at constant $V$ and $T$?
What is the effect on pressure if moles double at constant $V$ and $T$?
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Pressure doubles. More gas particles create greater pressure at constant volume and temperature.
Pressure doubles. More gas particles create greater pressure at constant volume and temperature.
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Identify the unit of the ideal gas constant $R$.
Identify the unit of the ideal gas constant $R$.
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L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.
L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.
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Identify the proportionality in Boyle's Law.
Identify the proportionality in Boyle's Law.
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Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.
Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.
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State the formula for Boyle's Law.
State the formula for Boyle's Law.
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$P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.
$P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.
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State the formula for the Ideal Gas Law.
State the formula for the Ideal Gas Law.
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$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.
$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.
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Identify the proportionality in Boyle's Law.
Identify the proportionality in Boyle's Law.
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Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.
Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.
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What does the variable $n$ represent in the Ideal Gas Law?
What does the variable $n$ represent in the Ideal Gas Law?
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Amount of substance in moles. Number of moles quantifies the amount of gas particles present.
Amount of substance in moles. Number of moles quantifies the amount of gas particles present.
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What is the effect on pressure if moles double at constant $V$ and $T$?
What is the effect on pressure if moles double at constant $V$ and $T$?
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Pressure doubles. More gas particles create greater pressure at constant volume and temperature.
Pressure doubles. More gas particles create greater pressure at constant volume and temperature.
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State the formula for Boyle's Law.
State the formula for Boyle's Law.
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$P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.
$P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.
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State the formula for the Ideal Gas Law.
State the formula for the Ideal Gas Law.
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$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.
$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.
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State the formula for Avogadro's Law.
State the formula for Avogadro's Law.
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$\frac{V_1}{n_1} = \frac{V_2}{n_2}$. Volume-moles relationship at constant pressure and temperature.
$\frac{V_1}{n_1} = \frac{V_2}{n_2}$. Volume-moles relationship at constant pressure and temperature.
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Find the temperature if $P = 1$ atm, $V = 22.4$ L, $n = 1$ mol, $R = 0.0821$.
Find the temperature if $P = 1$ atm, $V = 22.4$ L, $n = 1$ mol, $R = 0.0821$.
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273 K. Using $T = \frac{PV}{nR} = \frac{1 \times 22.4}{1 \times 0.0821}$.
273 K. Using $T = \frac{PV}{nR} = \frac{1 \times 22.4}{1 \times 0.0821}$.
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Convert 25°C to Kelvin.
Convert 25°C to Kelvin.
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298 K. Add 273.15 to convert Celsius to Kelvin.
298 K. Add 273.15 to convert Celsius to Kelvin.
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If $P = 2$ atm, $V = 5$ L, $T = 300$ K, find the moles of gas.
If $P = 2$ atm, $V = 5$ L, $T = 300$ K, find the moles of gas.
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0.406 mol. Using $n = \frac{PV}{RT} = \frac{2 \times 5}{0.0821 \times 300}$.
0.406 mol. Using $n = \frac{PV}{RT} = \frac{2 \times 5}{0.0821 \times 300}$.
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Find $n$ if $P = 1$ atm, $V = 24.4$ L, $T = 298$ K.
Find $n$ if $P = 1$ atm, $V = 24.4$ L, $T = 298$ K.
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1 mol. Using $n = \frac{PV}{RT} = \frac{1 \times 24.4}{298 \times 0.0821}$.
1 mol. Using $n = \frac{PV}{RT} = \frac{1 \times 24.4}{298 \times 0.0821}$.
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State the value of the ideal gas constant $R$.
State the value of the ideal gas constant $R$.
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0.0821 L atm mol$^{-1}$ K$^{-1}$. Standard value used in ideal gas calculations.
0.0821 L atm mol$^{-1}$ K$^{-1}$. Standard value used in ideal gas calculations.
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What does the variable $R$ represent in the Ideal Gas Law?
What does the variable $R$ represent in the Ideal Gas Law?
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Ideal gas constant. Universal constant relating gas properties, equal to 0.0821 L atm mol$^{-1}$ K$^{-1}$.
Ideal gas constant. Universal constant relating gas properties, equal to 0.0821 L atm mol$^{-1}$ K$^{-1}$.
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Calculate $T$ if $P = 3$ atm, $V = 5$ L, $n = 0.5$ mol, $R = 0.0821$.
Calculate $T$ if $P = 3$ atm, $V = 5$ L, $n = 0.5$ mol, $R = 0.0821$.
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366 K. Using $T = \frac{PV}{nR} = \frac{3 \times 5}{0.5 \times 0.0821}$.
366 K. Using $T = \frac{PV}{nR} = \frac{3 \times 5}{0.5 \times 0.0821}$.
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Identify the unit of volume in the Ideal Gas Law.
Identify the unit of volume in the Ideal Gas Law.
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Liters (L). Standard unit of volume in gas law calculations.
Liters (L). Standard unit of volume in gas law calculations.
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What happens to volume if both $P$ and $T$ double?
What happens to volume if both $P$ and $T$ double?
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Volume remains the same. Both pressure and temperature changes cancel out in the ideal gas law.
Volume remains the same. Both pressure and temperature changes cancel out in the ideal gas law.
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What happens to volume if temperature doubles at constant $P$ and $n$?
What happens to volume if temperature doubles at constant $P$ and $n$?
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Volume doubles. Direct relationship from Charles's Law at constant pressure.
Volume doubles. Direct relationship from Charles's Law at constant pressure.
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State the combined gas law formula.
State the combined gas law formula.
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$\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$. Relates initial and final states when moles remain constant.
$\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$. Relates initial and final states when moles remain constant.
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State the formula for Charles's Law.
State the formula for Charles's Law.
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$\frac{V_1}{T_1} = \frac{V_2}{T_2}$. Volume-temperature relationship at constant pressure and moles.
$\frac{V_1}{T_1} = \frac{V_2}{T_2}$. Volume-temperature relationship at constant pressure and moles.
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