Question

Given that ?H° for the thermochemical equation 2 SO2(g) + O2(g) ? 2SO3(g) is - 198 kJ, what is the enthalpy change for the decomposition of 1 mole of SO3 to give O2 and SO2, all in the gas state? Method: Write down the equation of the reaction required (decomposition of SO3 to give O2 and SO2): SO3(g) ? SO2(g) + 1/2O2(g) Compare this equation with the one for which the thermodynamic information is available, and decide what operations are necessary to make them identical. If you reverse a reaction, you must change the sign of ?H°. If you multiply a reaction through by a factor, you must multiply AH° by that factor also. Select one: a. + 99 kJ b. - 99 kJ c. - 198 kJ d. + 198 kJ e. 0 kJ

          Given that ?H° for the thermochemical equation
2 SO2(g) + O2(g) ? 2SO3(g)
is - 198 kJ, what is the enthalpy change for the decomposition of 1 mole of SO3
to give O2 and SO2, all in the gas state?
Method: Write down the equation of the reaction required (decomposition of SO3
to give O2 and SO2):
SO3(g) ? SO2(g) + 1/2O2(g)
Compare this equation with the one for which the thermodynamic information is
available, and decide what operations are necessary to make them identical.
If you reverse a reaction, you must change the sign of ?H°.
If you multiply a reaction through by a factor, you must multiply AH° by that factor
also.
Select one:
a. + 99 kJ
b. - 99 kJ
c. - 198 kJ
d. + 198 kJ
e. 0 kJ

Given that ?H° for the thermochemical equation
2 SO2(g) + O2(g) ? 2SO3(g)
is - 198 kJ, what is the enthalpy change for the decomposition of 1 mole of SO3
to give O2 and SO2, all in the gas state?
Method: Write down the equation of the reaction required (decomposition of SO3
to give O2 and SO2):
SO3(g) ? SO2(g) + 1/2O2(g)
Compare this equation with the one for which the thermodynamic information is
available, and decide what operations are necessary to make them identical.
If you reverse a reaction, you must change the sign of ?H°.
If you multiply a reaction through by a factor, you must multiply AH° by that factor
also.
Select one:
a. + 99 kJ
b. - 99 kJ
c. - 198 kJ
d. + 198 kJ
e. 0 kJ

Added by Jim F.

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