Figure 2 shows the displayed formula equation for the reaction of hydrogen sulfide with oxygen. In the reaction the energy released forming new bonds is 1034 kJ/mol greater than the energy needed to break existing bonds. Calculate the bond energy X for the bond. Use Figure 2 and the table above. – 6165

One thought on “Figure 2 shows the displayed formula equation for the reaction of hydrogen sulfide with oxygen. In the reaction the energy released forming new bonds is 1034 kJ/mol greater than the energy needed to break existing bonds. Calculate the bond energy X for the bond. Use Figure 2 and the table above. – 6165”

1. Step 1: Bonds Broken

   We break 4 bonds of energy 364 and 3 bonds of energy 498.
   So:
   4 × 364 = 1456
   3 × 498 = 1494
   Total bonds broken = 1456 + 1494 = 2950 kJ/mol

   Step 2: Bonds Formed

   We are told the total energy formed is:
   2950 + 1034 = 3984 kJ/mol

   Step 3: Equation Setup

   We are solving for the bond energy of X.
   Let’s say 4X + 4(464) = 3984
   So:
   4X + 1856 = 3984

   Step 4: Solving for X

   Subtract 1856 from both sides:
   4X = 2128
   Then divide by 4:
   X = 532 kJ/mol

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