1.) What pressure (in atm) is exerted by a column of isopropanol (C3H7OH) 295 m

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

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