gen chem 1 lab 8: molar mass of a vapor

boyles law formulas

P1V1 = P2V2 or P = 1/V

charles law

v1/v1 = t1/t2

amontons law

p1/p2=t1/t2

Amontons law applies when

the volume of a gas is constant

charles law applies when

the pressure is constant

percent error equation

((observed- expected)/expected ) x 100

van der waals equation

(p + (an²/V²)) + (V - nb) = nRT

dalton’s law of partial pressures

P1 + P2 = P3

according to boyles law at constant T and n

V is proportional to 1/P and P is proportion to 1/V

according the avogadros law at constant P and T

V is proportional to moles

according to charles law at constant P and n

V is proportional to T

ideal gas law with molar mass

PV = (m/M) RT

molar mass of gasses equation

M = mRT/ PV

determining mass of unknown

add aluminum secured w rubber band over a flask, record weight, add liquid to flask, add 350 mL of water and boiling chips to 600 mL beaker, heat water till boiling, then record temperature and pressure, clamp flask by hand in boiling water and wait till liquid has vaporized , then weigh to find mass, fill flask completely with water then pour into cylinder for volume

to identify a diatomic gas of researcher carried out the following experiment, she weighed an empty 3.8 L bulb, then filled it with the gas at 1.70atm and 24.0°C and waited again. The difference in mass was 7.5 g. Identify the gas.

N2 temperature

from the following data, calculate the molar mass of the unknown liquid: mass of vapor- 1.014 g, volume – 354 cm³, pressure – 741 torr, temperature – 99°C

M = 89.7 g/mol

density of gas equation

d = MP/ RT

calculate the molar mass of a gas is 2.80 g occupies 0.870 L at 685 torr and 37°C

90.8 g/mol

if an insufficient amount of liquid unknown has been used the experimental molar mass would’ve been

Lower

A sample of gas of mass 2.72 g occupies the volume of 639 mL at 27°C and one ATM pressure. What is the molar mass of the gas?

105 g/mol