Physics and Chemistry-Gas Laws

Question 1

how to remember the gas laws

Answer 1

Pink Can
Tight Be
Vagina Good

Question 2

How to remember the actual terms

Answer 2

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

Question 3

formula for boyels ideal gas law

Answer 3

P1 x V1 = P2 x V2

Question 4

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

Answer 4

Boyle’s gas law

Question 5

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

Answer 5

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

Question 6

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?

Answer 6

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

Question 7

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

Answer 7

Charles law

Question 8

Charles’ ideal gas Law:

states when temp increases, volume of gas does what?

Answer 8

increases

Question 9

Charles’ ideal gas Law:

how do u calculate Kelvin (k)

Answer 9

273 + celcius = K

Question 10

Charles’ ideal gas Law:

what is the formula

Answer 10

V1/T1 =V2/T2

Question 11

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

Answer 11

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

Question 12

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?

Answer 12

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

Question 13

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

Answer 13

Guy-Lussac’s

Question 14

Guy-Lussac’s Ideal gas Law:

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

Answer 14

increases

Question 15

Guy-Lussac’s Ideal gas Law:

whats is the formula

Answer 15

P1 / T1 = P2 / T2

Question 16

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

Answer 16

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

Question 17

Ex of whos law?

squeezing an ambu bag raised the pressure and decreases the volume

Answer 17

Boyle’s

Question 18

Ex of whos law?

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

Answer 18

Charles

Question 19

Ex of whos law?

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

Answer 19

Guy-Lussac’s

Question 20

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

Answer 20

Boyle’s

Question 21

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)

Answer 21

Daltons law of partial pressures

Question 22

Daltons law of partial pressures:

how do you calculate the partial pressure of a gas

Answer 22

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

Question 23

Daltons law of partial pressures:

how is it applied to us

Answer 23

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

Question 24

Daltons law of partial pressures:

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

Answer 24

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)

Question 25

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)

Answer 25

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

Question 26

Daltons law of partial pressures: question

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

Answer 26

O2 21%

0.21 x 550 = 116mmHg

Question 27

Daltons law of partial pressures Question

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

Answer 27

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

0.5 x 760 = 38 mmHg

Question 28

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

Answer 28

Avogadro’s number and hypothesis

Question 29

Avogadro’s number:

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

Answer 29

6.022 x 10^23

Question 30

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?

Answer 30

22.4 L

Question 31

Avogadro’s hypothesis: problem

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

Answer 31

22.4L x 2= 44.8L

Question 32

Avogadro’s hypothesis: Problem

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

Answer 32

0.5 x 22.4L = 11.2L