Question

Nitrogen dioxide, NO2(

g. Hf = 33.84 kJ/mol), is decomposed according to the following reaction: What is the enthalpy change when 2.50 mol of nitrogen dioxide decomposes? 13.5 kJ of energy released 13.5 kJ of energy absorbed 84.6 kJ of energy released 84.6 kJ of energy absorbed

Answer 1

C.

Step-by-step explanation:

took the test

Answer 2

Answer:84.6 kJ of energy released when 2.50 moles of nitrogen dioxide is decomposed.

Step-by-step explanation:

`N(g)+O_2(g)\rightarrow NO_2(g),\Delta H_f=33.84 kJ/mol`

Energy released when 1 mole of
`NO_2` is formed = 33.84 kJ

And When 1 mole of
`NO_2` is decomposed it gives out 33.84 kJ of energy.

Energy released when 2.50 moles of nitrogen dioxide is decomposed:

`33.84 kJ* 2.50 =84.6 kJ`

84.6 kJ of energy released when 2.50 moles of nitrogen dioxide is decomposed.