gas the fucking laws

Question 1

What does STP stand for in chemistry?

Answer 1

Standard Temperature and Pressure

Question 2

What is the standard temperature at STP?

Answer 2

0°C or 273.15 K

Question 3

What is the standard pressure at STP?

Answer 3

1 atm = 101.325 kPa = 760 mmHg = 760 torr = 14.7 psi

Question 4

What is the molar volume of an ideal gas at STP?

Answer 4

22.4 L per mole of gas

Question 5

What is Boyle’s Law?

Answer 5

P₁V₁ = P₂V₂ — Pressure and volume are inversely related when temperature and moles are constant.

Question 6

When does Boyle’s Law apply?

Answer 6

When temperature and amount of gas are constant.

Question 7

What is Charles’s Law?

Answer 7

V₁/T₁ = V₂/T₂ — Volume and temperature are directly related when pressure and moles are constant.

Question 8

When does Charles’s Law apply?

Answer 8

When pressure and amount of gas are constant.

Question 9

What is Gay-Lussac’s Law?

Answer 9

P₁/T₁ = P₂/T₂ — Pressure and temperature are directly related when volume and moles are constant.

Question 10

When does Gay-Lussac’s Law apply?

Answer 10

When volume and amount of gas are constant.

Question 11

What is Avogadro’s Law?

Answer 11

V₁/n₁ = V₂/n₂ — Volume is directly proportional to the number of moles when pressure and temperature are constant.

Question 12

When does Avogadro’s Law apply?

Answer 12

When temperature and pressure are constant.

Question 13

What is the Combined Gas Law?

Answer 13

(P₁V₁)/T₁ = (P₂V₂)/T₂ — Relates pressure, volume, and temperature when moles are constant.

Question 14

When does the Combined Gas Law apply?

Answer 14

When the number of moles of gas is constant.

Question 15

What is the Ideal Gas Law?

Answer 15

PV = nRT — Relates pressure, volume, moles, temperature, and gas constant for an ideal gas.

Question 16

What is Dalton’s Law of Partial Pressures?

Answer 16

P_total = P₁ + P₂ + P₃ + … — Total pressure equals the sum of the partial pressures of all gases in the mixture.

Question 17

How do you find partial pressure using mole fraction?

Answer 17

P₁ = X₁ × P_total, where X₁ = (moles of gas 1) / (total moles of gas).

Question 18

When does Dalton’s Law apply?

Answer 18

When gases are mixed in the same container.

Question 19

What is Graham’s Law of Effusion?

Answer 19

Rate₁ / Rate₂ = √(M₂ / M₁) — Lighter gases effuse or diffuse faster than heavier gases.

Question 20

When does Graham’s Law apply?

Answer 20

When comparing the rates of effusion or diffusion of two gases.

Question 21

What does Graham’s Law describe?

Answer 21

The relationship between the speed of gas particles and their molar masses.

Question 22

What is the formula for Graham’s Law using rate?

Answer 22

Rate₁ / Rate₂ = √(M₂ / M₁)

Question 23

How is rate related to molar mass in Graham’s Law?

Answer 23

Rate is inversely proportional to the square root of molar mass.

Question 24

What is the formula for Graham’s Law using distance?

Answer 24

Distance₁ / Distance₂ = √(M₂ / M₁)

Question 25

How is distance related to molar mass in Graham’s Law?

Answer 25

Distance is inversely proportional to the square root of molar mass.

Question 26

What is the formula for Graham’s Law using time?

Answer 26

Time₂ / Time₁ = √(M₂ / M₁)

Question 27

How is time related to molar mass in Graham’s Law?

Answer 27

Time is directly proportional to the square root of molar mass.

Question 28

When using time instead of rate, how should you set up Graham’s Law?

Answer 28

The slower gas’s time over the faster gas’s time = √(heavier M / lighter M)

Question 29

Do you need specific units for the Ideal Gas Law?

Answer 29

Yes, pressure must be in atm, volume in liters, temperature in Kelvin, and moles in moles.

Question 30

In other gas laws, when should temperature be converted to Kelvin?

Answer 30

Temperature must always be converted to Kelvin in gas laws where temperature is involved, but the rest of the units can remain the same.