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brilliants [131]
3 years ago
9

The decomposition of N I 3 to form N 2 and I 2 releases − 290.0 kJ of energy. The reaction can be represented as 2N I 3 (s)→ N 2

(g)+3 I 2 (g), ΔH rxn =−290.0 kJ Find the change in enthaply when 10.0 g of N I 3 decomposes. Express your answer to three significant figures and include the appropriate units.
Chemistry
1 answer:
ella [17]3 years ago
3 0

Answer:

The change in enthaply when 10.0 g of nitrogen triiodide decomposes is -3.67 kJ.

Explanation:

2NI_3 (s)\rightarrow N_2 (g)+3 I_2 (g), \Delta H_{rxn} =-290.0 kJ

Enthalpy of the reaction when 2 moles of nitrogen triiodide decomposed =\Delta H_{rxn}

\Delta H_{rxn} = -290.0 kJ

Enthalpy of the reaction when 1 moles of nitrogen triiodide decomposed :

\Delta H=\frac{\Delta H_{rxn}}{2}=\frac{-290.0 kJ}{2} =-145.0 kJ

Mass of nitrogen triiodide decomposed = 10.0 g

Moles of nitrogen triiodide = \frac{10.0 g}{395 g/mol}=0.02532 mol

Change in enthaply when 0.02532 moles of nitrogen triiodide decomposed:

\Delta H\times 0.02532=-145 kJ\times 0.02532=-3.67 kJ

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