Can someone help me with the calculations? I also need to find: l) Room pressure

Question

Can someone help me with the calculations?
I also need to find:
l) Room pressure in atmospheres
m) Volume of the flask in liters
n) Temperature of the lab gas in Kelvins
o) Number of moles of lab gas from the ideal gas law
p) Molar mass of the lab gas

DATA a) Mass of the task, stopperand air 1181 b) Temperature in the room. c) Mass of the Alask, stopperand lab gas 113 443 d) Temperature in the hood. 2 Don e) Volume of the flask measured by the cylinder D Room pressure in mmHg g) Density of dry air from the chart CALCULATIONS b) Mass of the air in the flask B) Mass of the flask and stopper without air j Mass of the lab gas sample 1) Density of the lab gas in grams per liter

Explanation / Answer

h) volume of flask measured by cylinder = 260 ml = 0.260 L

Density of dry air = 1.193 g/L

Mass of air in flask = Density*volume = 1.193*0.260 = 0.310 g

i) Mass of flask and stopper without air = Mass of flask with air - mass of air = 118.111 g - 0.310 g = 117.801 g

j) Mass of lab gas sample = Mass of flask with lab gas sample - Mass of flask and stopper without air

= 117.993 g - 117.801 g = 0.192 g

k) Density of lab gas = Mass of lab gas/Volume of flask = 0.192 g/0.260 L = 0.738 g/L

l) Room pressure in atm: Room pressure in torr = 760 torr

760 torr = 1 atm.

So Room pressure in atm = 1 atm

m) Volume of flask in litres: Volume of flask = 260 ml

1000 ml = 1L

So, 260 ml = 260/1000 = 0.260 L

Volume of flask in litres = 0.260 L

n) Temperature of lab gas in Kelvin:

Temperature of lab gas = temperature of room = 23.7 oC

Temperature in Kelvin = Temperature in oC + 273 = 23.7+273 = 296.7 K

Temperature of lab gas in Kelvin = 296.7 K

o) Number of moles of lab gas from the ideal gas law:

Ideal gas law = PV = nRT

n = PV/RT

P = pressure = 1 atm

V = volume = 260 ml = 0.260 L

R = 0.082 L atm/mol K

T = 23.7 oC = 296.7 K

n = (1 atm) (0.260 L)/[(0.082 L atm/mol K)(296.7 K)]

= 0.0106 mol

Number of moles of lab gas = n = 0.0106 mol

p) Mass of lab gas = 0.192 g

number of moles = 0.0106 mol

Molar mass = mass/number of moles = 0.192 g/0.0106 mol = 18.11 g/mol

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