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The enthalpy of formation of SO2(g) is 296.7 kJ. The energy required for the decomposition of 2 mole of SO2(g) into sulphur(rhombic) and gaseous O2 is (a) 148.35 kJ (b) 296.7 kJ (c) 593.4 kJ (d) 148.35 kJ choose and explain

The enthalpy of formation of SO2(g) is 296.7 kJ. The energy required for the decomposition of 2 mole of SO2(g) into sulphur(rhombic) and gaseous O2 is


 (a) 148.35 kJ (b) 296.7 kJ (c) 593.4 kJ (d) 148.35 kJ


choose and explain


 

Grade:12

1 Answers

Vikas TU
14149 Points
7 years ago

So,

S + O2 --> SO2 DeltaH = +296.7

You want Delta H for the equation:

2 SO2 --> 2S + 2 O2

Since you are flipping the equation, change it sign. Since you have 2 mol SO2, multiply the Delta H by 2 to get:

Delta H = -593.4 kJ

Now, I''m guessing that your original Delta H value should have a negative sign, so that the answer to the question would actually be +593.4 kJ.

 

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