Answer :
Given:
Enthalpy of decomposition of NO2 = 33.84 kJ/mol
To determine:
Enthalpy change when 2.5 moles of NO2 decomposes
Explanation:
The decomposition of NO2 is represented as:
2NO2(g) → N2(g) + 2O2(g)
Enthalpy change when 1 mole of NO2 decomposes is 33.84 kJ
therefore the enthalpy change corresponding to the decomposition of 2.50 moles of NO2 = 33.84 kJ * 2.40 moles/ 1 mole = 81.22 kJ
Ans: ΔH(decomposition) = 81.22 kJ
Answer:
The enthalpy change when 2.50 mol of nitrogen dioxide decomposes is 84.6 kJ/mol.
Explanation:
Enthalpy of the formation of [tex]NO_2=33.84 kJ/mol[/tex]
[tex]\frac{1}{2}N_2+O_2\rightarrow NO_2,\Delta H_f=33.84 kJ/mol[/tex]
Enthalpy of decomposition when one mol of nitrogen-dioxide decomposes.
[tex]NO_2\rightarrow \frac{1}{2}N_2+O_2,\Delta H_d=-33.84 kJ/mol[/tex]
When 1 mol of [tex]NO_2[/tex] decomposes it gives = -33.84 kJ/mol
When 2.50 mol of nitrogen-dioxide decomposes to give:
[tex]2.5 \times -33.84 kJ/mol=-84.6kJ/mol[/tex]
The enthalpy change when 2.50 mol of nitrogen dioxide decomposes is 84.6 kJ/mol.