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juin [17]
3 years ago
13

According to the following thermochemical equation, if 951.1 g of NO 2 is produced, how much heat is released at constant pressu

re? 2NO(g) + O2(g) 2NO 2(g); DH -114.4 kJ
Chemistry
1 answer:
nordsb [41]3 years ago
4 0

Answer:

The amount of released is 1,182 kJ.

Explanation:

When heat is released at constant pressure, this change in energy is known as enthalpy (ΔH°) of the reaction. Enthalpy is an extensive property, so it depends on the amount of reacting material. Let's take a look at the provided equation:

2 NO(g) + O₂ ⇄ 2 NO₂(g)   ΔH° = -114.4 kJ

Since this equation is balanced with 2 moles of NO₂(g), we can say that 114.4 kJ are released every 2 moles of NO₂(g) produced. By convention, when enthalpies are negative, it means that energy is <em>released</em> and the reaction is exothermic. Conversely, positive enthalpies mean energy is <em>absorbed</em> and the reaction is endothermic.

We can calculate the amount of energy released taking into account the previous relationship (-114.4 kJ/2 moles of NO₂(g)), the mass of NO₂(g) produced (951.1g) and its molar mass (46.00g/mol). The calculations would be:

951.1g.\frac{1molNO_{2} }{46.00g} .\frac{-114.4kJ}{2molesNO_{2} } =-1,182kJ

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