1.) What pressure (in atm) is exerted by a column of isopropanol (C3H7OH) 295 m
ID: 920874 • Letter: 1
Question
1.) What pressure (in atm) is exerted by a column of isopropanol (C3H7OH) 295 m high? The density of isopropanol is 0.785 g/cm^3.
2.) Propane (C3H8) burns in oxygen to produce carbon dioxide gas and water vapor.
a.) Write a balanced equation for this reaction. Include all reaction states.
b.)Calculate the number of liters of carbon dioxide measured at STP that could be produced from 7.45 g of propane.
3.) The empirical formula of a compound is CH. At 200 degrees C, 0.073 g of this compound occupies 97.2 mL at a pressure of 0.74 atm. What is the molecular formula of the compound?
Explanation / Answer
1) Pressure = density x g x height
Given,
column height = 295 m
density = 0.785 g/cm^3 = 785 kg / m^3
=> Pressure = 785 x 9.8 x 295 = 2269435 Pa = 22.69 bar
2) Balanced Equation for the reaction:
C3H8 + 5O2 -----> 3CO2 + 4H2O
Given,
Mass of proprane = 7.45 g
We know that molar mass of propane = 44.1 g / mol
=> Moles of Propane = 7.45 / 44.1 = 0.17 moles
According to the stoichiometry of the reaction 1 mole of propane combusts to produce 3 moles of CO2
=> Moles of CO2 produced = 0.17 x 3 = 0.51 moles
1 mole of CO2 at STP occupies 22.4 liters
=> Volume occupied = 22.4 x 0.51 = 11.4 liters
3)
We know that PV = nRT
P = 0.74 atm
V = 92.7 mL = 0.0972 L
R = 00821
T = 200 C = 473 K
=> 0.74 x 0.0972 = n x 0.0821 x 473
=> n = 1.85 x 10^-3 moles
Mass = Moles x Molar Mass
=> 0.073 = 1.85 x 10^-3 x Molar Mass
=> Molar Mass = 39.4 g
Emperical Mass of CH = 12+1 = 13
X = 39.4 / 13 = 3
Molecular Formula of compound = C3H3
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.