Answer:
a) 0.957895 atm
b) 372.05 K
c) 0.524 grams
d) 0.00725 moles
e) Molar mass gas = 30.54 g/mol
Explanation:
Step 1: Data given
Mass of the flask = 53.256 grams
Volume = 5 mL
Temperature of water = 98.9 °C = 372.05 K
Mass obtained = 53.78 grams
The volume of the flask is known to be 231.1 mL = 0.2311 L
The absolute atmospheric pressure in the laboratory that day is 728 mm Hg.
Step 2: Calculate the mass of the gas
Mass gas = 53.780 - 53.256 = 0.524 grams
Step 3: Calculate moles
p*V = n*R*T
⇒with p = the pressure = 0.957895 atm
⇒with V = the volume = 0.2311 L
⇒with n = the number of moles gas = TO BE DETERMINED
⇒with R = the gas constant = 0.08206 L*atm/mol * K
⇒with T = the temperature = 372.05 K
n = (p*V)/(R*T)
n= (0.957895 * 0.2311) / (0.08206 * 372.05)
n = 0.00725 moles
Step 4: Calculate mass of the gas
Molar mass = mass / moles
Molar mass gas = 0.524 grams . 0.00725 moles
Molar mass gas = 30.54 g/mol
