A compound has the empirical formula CHCI. A 256-mL flask, at 373 K and 750. tor

Question

A compound has the empirical formula CHCI. A 256-mL flask, at 373 K and 750. torr. contains 0.800 g of the gaseous compound. Give the molecular formula The heat capacity of a bomb calorimeter was determined by burning 4.73 g methane. C4, (energy of combustion = -802 kJ/mol) in the bomb. The temperature changed by 10.8 degree C. What is the heat capacity of the bomb? A 12.6 g sample of acetylene. C2H2, produced a temperature increase of 16.9 degree C in the same calorimeter. What is the energy of combustion of acetylene (in kJ/mol)? For the following reaction: H-C C-H + O=O O=C=O + .H O H For the combustion of 1 mole of acetylene (C2H3), balance the reaction by putting the correct number to the left of the Lewis structure. Using the delta H degree t, values listed at the end of this exam, estimate AH for this reaction. Using the bond energy values listed at the end of this exam, estimate delta H for this reaction. The delta H for this reaction has been experimentally determined to be -1300 kJ/mol. What method (standard enthalpy of formation or bond energies) does a better job of predicting the AH for this reaction? For the following Lewis structure: Assuming an overall charge of 0 for the molecule, draw in all of the tone pairs of electrons. Assign formal charges for all of the carbon, oxygen and nitrogen atoms on the structure Indicate which atom above is sp2 hybridized. Draw the other resonance structure for the molecule in which the overall charge of the molecule Is still 0.

Explanation / Answer

4.          Given V = 256 ml,     p = 750 torr   m = 0.800g T = 373 K

                         PV = mRT/M

                        M = mRT/PV =   (0.800 g) * (0.0821) (373) /(750 torr) (256 ml)

                   Converting torr into Atm   1Atm = 760 torr. And change ml to Liters.

                       M = 95.697.

  it is a gaseous compound. It may be C2H4Cl2.

5 .     Given mass = m = 12.6 g of Acetylene.

            moles =   n    = 12.6 /26.04 = 0.484 moles.

                         T = 16.9 = 290.05 Kelvin.

                   heat of combustion = nCdT = 0.484* 44.04 Jmole*k * 290.05 = 6.18 KJ /mole.

6.         a. C2H2    +    5/2 O2   ------------

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