# Physics and Chemistry-Gas Laws Flashcards Preview

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Flashcards in Physics and Chemistry-Gas Laws Deck (32)
1
Q

how to remember the gas laws

A

Pink Can
Tight Be
Vagina Good

2
Q

How to remember the actual terms

A

Pressure (constant) Charles
Temp (constant) Boyles
volume (constant) Guy-lusac

3
Q

formula for boyels ideal gas law

A

P1 x V1 = P2 x V2

4
Q

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

A

Boyle’s gas law

5
Q

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

A

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

6
Q

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?

A
```P1 x V1 = P2 x V2
1900psi x (X) = 14.7psi x 660L
X= (14.7psi x 660L) / 1900psi = 5.1L```
7
Q

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

A

Charles law

8
Q

Charles’ ideal gas Law:

states when temp increases, volume of gas does what?

A

increases

9
Q

Charles’ ideal gas Law:

how do u calculate Kelvin (k)

A

273 + celcius = K

10
Q

Charles’ ideal gas Law:

what is the formula

A

V1/T1 =V2/T2

11
Q

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

A

V1/T1 = V2/T2
1L / 273K = X / 373K
(1L /273K) x 373k = X
X= 1.366 L

12
Q

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?

A

V1 / T1 = V2 / T2
5L / 323k = X / 273k
(5L / 323k) / 273 = X
X = 4.23L

13
Q

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

A

Guy-Lussac’s

14
Q

Guy-Lussac’s Ideal gas Law:

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

A

increases

15
Q

Guy-Lussac’s Ideal gas Law:

whats is the formula

A

P1 / T1 = P2 / T2

16
Q

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

A

P1 / T1 = P2 / T2
2500psi / 333k = X / 288k
(2500psi / 333k) x 288k = X
X = 2160psi

17
Q

Ex of whos law?

squeezing an ambu bag raised the pressure and decreases the volume

A

Boyle’s

18
Q

Ex of whos law?

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

A

Charles

19
Q

Ex of whos law?

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

A

Guy-Lussac’s

20
Q

Ex of whos law?
During inspiration when breathing spontaneously, intrapulmonary falls and volume increases. during expiration, intrapulmonary pressure increase and volume decrease

A

Boyle’s

21
Q

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)

A

Daltons law of partial pressures

22
Q

Daltons law of partial pressures:

how do you calculate the partial pressure of a gas

A

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

23
Q

Daltons law of partial pressures:

how is it applied to us

A

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

24
Q

Daltons law of partial pressures:

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

A

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)

25
Q

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)

A

N20-> 0.70 x 760 = 532 mmHg
O2-> 0.30 x 760 = 228 mmHg
532 + 228 = 760mmHg

26
Q

Daltons law of partial pressures: question

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

A

O2 21%

0.21 x 550 = 116mmHg

27
Q

Daltons law of partial pressures Question

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

A

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

0.5 x 760 = 38 mmHg

28
Q

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

A

29
Q

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

A

6.022 x 10^23

30
Q

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

A

22.4 L

31
Q

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

A

22.4L x 2= 44.8L

32
Q