Consider the following thermochemical equation for the combustion of acetone, C3H6O, the main ingredient in nail polish remover: C3H6O(l)+4O2(g)→3CO2(g)+3H2O(g) ΔH∘rxn=−1790kJ If a bottle of nail polish remover contains 174 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL.

number of structural isomers possible in C3H6O A)9 B)6 C)5 D ) View Solution. Q2.

Complete combustion of 1 mole of acetone, C3H6O, releases 1790 kJ of heat: C3H6O (l) + 4O2 (g) → 3CO2 (g) + 3H2O (l) ΔH° = -1790 kJ Using data from tables that list standard enthalpy of formation of O2(g), CO2(g), and H2O(l), Show the calculations to determine the enthalpy of formation of acetone

A structural isomer, also known as a constitutional isomer, is one in which two or more organic compounds have the same molecular formulas but different structures. and in this given molecule i.e. C 3 H 6 O having 9 structures as follows:(refer image)

A catalyst was created to convert C3H8O into C3H6O through a gas-phase reaction at 450 K and 0.75 bar: C3H8O = C3H6O + H2 The feed is C3H8O and N2 (an inert) at a 1:4 mole ratio. At thermodynamic equilibrium, determine percent conversion of C3H8O.

A chemist combined chloroform (CHCl3)(CHCl3) and acetone (C3H6O)(C3⁢H6O) to create a solution where the mole fraction of chloroform, ?chloroform,χchloroform, is 0.1870.187. The densities of chloroform and acetone are 1.48 g/mL1.48 g/mL and 0.791 g/mL,0.791 g/mL, respectively. Calculate the molarity of the solution.

Solution for A 9.50 % by mass solution of acetone (C3H6O) in water has a density of 0.9849 g/mL at 20°C. What is the molarity of this solution?

The complete combustion of 1 mole of acetone (C3H6O) releases 1790 kJ of heat: C3H6O + 4 O2 → 3 CO2 + 3 H2O Using this information together with the standard heats of formation table, calculate the enthalpy of formation of acetone (CaHsO).

The combustion of liquid acetone, C3H6O will produce gaseous carbon dioxide and water. Use the following thermochemical equations to calculate the standard enthalpy of combustion for one mole acetone.

What is the mole fraction of acetone, C3H6O, in the vapor phase from a solution consisting of a mixture of acetone and ethyl acetate, CH3COOCH2CH3, at 30.00 °C, if the total pressure above the solution is 202.2 torr? The vapor pressures of pure acetone and NaN at 30.00 °C are 285.0 torr and 118.0 torr, respectively.