The fundamental vibrational frequencies for 1H2and 14N2 are 4401 and 2359 cm1, r

Question

The fundamental vibrational frequencies for 1H2and 14N2 are 4401 and 2359 cm1, respectively, and De for this molecules is 7.677×1019 and 1.593×1018 J respectively.

Part A

Using this information, calculate the bond energy of 1H2.

Express your answer to four significant figures and include the appropriate units.

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Part B

Calculate the bond energy of 14N2.

Express your answer to four significant figures and include the appropriate units.

The fundamental vibrational frequencies for 1H2and 14N2 are 4401 and 2359 cm1, respectively, and De for this molecules is 7.677×1019 and 1.593×1018 J respectively.

Part A

Using this information, calculate the bond energy of 1H2.

Express your answer to four significant figures and include the appropriate units.

EH2 =

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Part B

Calculate the bond energy of 14N2.

Express your answer to four significant figures and include the appropriate units.

EN2 =

Explanation / Answer

The expression for Energy, En=h(n+1/2)- [(h)2(n+1/2)2]/4De

For, fundamental vibration, n=0

Therefore, E0=h/2- (h)2/16De

Where, h=Planck’s constant =6.626x10-34Js

and =fundamental frequency

Bond Energy =D0= De-E0

Part A: For H2:      1/=4401cm-1 ; De=7.677x10-19J

                                =c/ =1.32x1014s-1

E0= (6.626x10-34) (1.32x1014) /2- [(6.626x10-34) (1.32x1014)]2/16(7.677x10-19)

E0= 4.3108x10-20J

Therefore, Bond Energy =D0= De-E0 =7.677x10-19 - 4.3108x10-20 J =7.246 x10-19 J

Part B: For N2:      1/=2359cm-1 ; De=1.593 x10-18J

                                =c/ =7.07x1013s-1

E0= (6.626x10-34) (7.07x1013) /2- [(6.626x10-34) (7.07x1013)]2/16(1.593x10-18)

E0= 2.333x10-20J

Therefore, Bond Energy =D0= De-E0 =1.593 x10-18 - 2.333x10-20 J =1.569 x10-18 J

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