how to remember the gas laws

Pink Can

Tight Be

Vagina Good

How to remember the actual terms

Pressure (constant) Charles

Temp (constant) Boyles

volume (constant) Guy-lusac

formula for boyels ideal gas law

P1 x V1 = P2 x V2

whose law states pressure is inversely proportional to volume at a constant temp

Boyle’s gas law

Boyle’s Gas Law:

if a pressurized cylinder is opened and slowly emptied so that temp does not change, the volume of gas released from the cylinder can be estimated

basically the law explains why a large volume of gas is released from a pressurized cylinder

Boyle’s Gas Law: question

an E cylinder has a full pressure of 1900psi. we know that a full E cylinder will expand to approx 660L. what is the volume in the E cylinder?

P1 x V1 = P2 x V2 1900psi x (X) = 14.7psi x 660L X= (14.7psi x 660L) / 1900psi = 5.1L

who’s law states volume is directly proportional to the absolute temp (K) at a constant pressure?

Charles law

Charles’ ideal gas Law:

states when temp increases, volume of gas does what?

increases

Charles’ ideal gas Law:

how do u calculate Kelvin (k)

273 + celcius = K

Charles’ ideal gas Law:

what is the formula

V1/T1 =V2/T2

Charles’ ideal gas Law: question

a balloon is filled with air and has a pressure of 1 atm, and a temp of 0C, and a volume of 1 L. what is the volume of the balloon at 100C and a pressure of 1 Atm

V1/T1 = V2/T2

1L / 273K = X / 373K

(1L /273K) x 373k = X

X= 1.366 L

Charles’ ideal gas Law: question

a bouncy ball has a temp of 50 C in the sun and a volume of 5L w/ a pressure of 760mmHg. if the pressure remains the same what is the volume at 0 C?

V1 / T1 = V2 / T2

5L / 323k = X / 273k

(5L / 323k) / 273 = X

X = 4.23L

who’s law states pressure is directly proportional to an absolute temp (k) if volume is constant?

Guy-Lussac’s

Guy-Lussac’s Ideal gas Law:

states that when the temp increases in a container with a constant volume what happens to pressure

increases

Guy-Lussac’s Ideal gas Law:

whats is the formula

P1 / T1 = P2 / T2

Guy-Lussac’s Ideal gas Law: question

A E cylinder was left in the sun on the loading deck of a hospital. It has a temp of 60 C and a pressure of 2500psi. what will the pressure be in the cylinder at a temp of 15 C

P1 / T1 = P2 / T2

2500psi / 333k = X / 288k

(2500psi / 333k) x 288k = X

X = 2160psi

Ex of whos law?

squeezing an ambu bag raised the pressure and decreases the volume

Boyle’s

Ex of whos law?

the inflatable cuff of an LMA expands when placed into an autoclave

Charles

Ex of whos law?

as the N20 cylinder empties the pressure of the tank decreases even N20 is present

Guy-Lussac’s

Ex of whos law?

During inspiration when breathing spontaneously, intrapulmonary falls and volume increases. during expiration, intrapulmonary pressure increase and volume decrease

Boyle’s

who’s law of partial pressures states: the total pressure in a mixture of gases is equal to the sum of the pressures of the individual gases (each gas is said to exert a partial pressure)

Daltons law of partial pressures

Daltons law of partial pressures:

how do you calculate the partial pressure of a gas

by multiplying the % gas (fractional concentration) times atmospheric pressure

Daltons law of partial pressures:

how is it applied to us

it allows us to calculate the partial pressure of a gas if the % concentration is known

Daltons law of partial pressures:

it the atmosphere at sea level what are the partial pressures of O2 and N2

O2 21% so 0.21 x 760 = 160 mmHg

N2 79% so 0.79 x 760 = 600 mmHg

160 + 600 = 760 mmHG (which is atm pressure)

Daltons law of partial pressures: question

what are the partial pressures of N20 and O2 is they are delivered to a pt in a 70%/30% N2O/O2 mixture (assume sea level)

N20-> 0.70 x 760 = 532 mmHg

O2-> 0.30 x 760 = 228 mmHg

532 + 228 = 760mmHg

Daltons law of partial pressures: question

what is the partial pressure of O2 in the mountains where atm pressure is 550mmHg

O2 21%

0.21 x 550 = 116mmHg

Daltons law of partial pressures Question

what is the partial pressure of CO2 if its concentration in the ET gases is 5%

if they don;t specify always use sea level atm pressure

0.5 x 760 = 38 mmHg

who number/ hypothesis described the relationship b/t the amount of gas and volume of gas

Avogadro’s number and hypothesis

Avogadro’s number:

states the number of molecules in 1 mole of a substance is what?

6.022 x 10^23

Avogadro’s hypothesis:

states that one mole of a gas at standard temp (O C) and a standard pressure (1 atm) (STP) occupies a volume of what?

22.4 L

Avogadro’s hypothesis: problem

2 moles of gaseous N2O occupy what volume under standard conditions?

22.4L x 2= 44.8L

Avogadro’s hypothesis: Problem

one-half mole of O2 occupies what volume under standard conditions

0.5 x 22.4L = 11.2L