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zysi [14]
3 years ago
15

Part b solid lithium metal and diatomic nitrogen gas react spontaneously to form a solid product. give the balanced chemical equ

ation (including phases) that describes this reaction. indicate the phases using abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively.
Chemistry
1 answer:
dimaraw [331]3 years ago
3 0

Lithium metal which is an alkali metal belongs to the Group I of the periodic table reacts spontaneously with nitrogen, (which remains in gaseous form at room temperature) to form solid lithium nitride (Li_{3}N). The reaction can be shown as- 6Li (s) + N_{2}(g) = 2Li_{3}N(s). This is the only example of alkali nitride in chemistry. The other alkali nitrides are either not stable or does not exist in solid form at room temperature.

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30 feet /second

Explanation:

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Which of the following statements best describes the relationships between carrying captivity in population size
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3 years ago
Part a use these data to calculate the heat of hydrogenation of buta-1,3-diene to butane. c4h6(g)+2h2(g)→c4h10(g)
Reptile [31]

<u>Answer:</u> The heat of hydrogenation of the reaction is coming out to be 234.2 kJ.

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as \Delta H

The equation used to calculate enthalpy change is of a reaction is:

\Delta H_{rxn}=\sum [n\times \Delta H_{(product)}]-\sum [n\times \Delta H_{(reactant)}]

For the given chemical reaction:

C_4H_6(g)+2H_2(g)\rightarrow C_4H_{10}(g)

The equation for the enthalpy change of the above reaction is:

\Delta H_{rxn}=[(1\times \Delta H_{(C_4H_{10})})]-[(1\times \Delta H_{(C_4H_6)})+(2\times \Delta H_{(H_2)})]

We are given:

\Delta H_{(C_4H_{10})}=-2877.6kJ/mol\\\Delta H_{(C_4H_6)}=-2540.2kJ/mol\\\Delta H_{(H_2)}=-285.8kJ/mol

Putting values in above equation, we get:

\Delta H_{rxn}=[(1\times (-2877.6))]-[(1\times (-2540.2))+(2\times (-285.8))]\\\\\Delta H_{rxn}=234.2J

Hence, the heat of hydrogenation of the reaction is coming out to be 234.2 kJ.

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