2B - Analysis IR  /14

             For the following reaction:

                                        A     +     B     à     C    +    H₂O

	A	B	C
Molecular formula	CH3OH  [1]	CH3COOH  [1]	CH3COOCH3  [1]
IR Spectra
	OH peak only, no C=O peak  [1]	OH peak and C=O peak  [1]	C=O peak only, no OH peak  [1]

                1)  Identify A, B and C given the information above.  [6]

                        A - Methanol  B - Ethanoic acid  C - Methyl Ethanoate

                2)  Write a balanced equation for the reaction above.  [1]

                                        CH₃OH     +     CH₃COOH     à     CH₃COOCH₃    +    H₂O

                3)  1.60g of A reacted with 3.50g of B to make 3.50g of C. 

                     Calculate the % yield for the reaction. [6]

                        Moles A / CH₃OH = 0.0500 [1]      Moles of B / CH₃COOH = 0.0583  [1] 

                        A / CH₃OH is limiting reagent  [1]

                        Moles C / CH₃COOCH₃ that could be made = 0.0500  [1]

                        Moles C / CH₃COOCH₃ that was actually made = 0.0473  [1]

                        % Yield = (0.0473 / 0.0500) x 100  =  94.6% [1]

                4)  Calculate the atom economy for the production of C [1]

                        Atom economy =      74      x  100     =    80.4%

                                                    (74+18)