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AlladinOne [14]
3 years ago
13

PLEASE HELP I AM FAILING SCIENCE!!!

Chemistry
1 answer:
kherson [118]3 years ago
8 0

Answer: B. Mg

Explanation:

Ionization energy is the energy required for the removal of valence electron from an isolated gaseous atom.

Ionization energy increases as we move across the period as the atomic size decreases as the electrons are being added to the same energy level.

Ionization energy decreases as we move down the group as the atomic size increases due to the addition of shells.

As magnesium (Mg) lies to the right of Sodium (Na) and Poatssium (K) and Calcium (Ca) lies below Magnesium (Mg), Mg has the highest ionization energy.

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Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2H2S(g) 3O2(g)2H2O(l) 2SO2
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Answer:

\Delta _rH=-1124.14kJ/mol

Explanation:

Hello!

In this case, since the standard enthalpy change for a chemical reaction is stood for the enthalpy of reaction, for the given reaction:

2H_2S(g) +3O_2(g)\rightarrow 2H_2O(l) +2SO_2(g)

We set up the enthalpy of reaction considering the enthalpy of formation of each species in the reaction at the specified phase and the stoichiometric coefficient:

\Delta _rH=2\Delta _fH_{H_2O,liq}+2\Delta _fH_{SO_2,gas}-2\Delta _fH_{H_2S,gas}-3\Delta _fH_{O_2,gas}

In such a way, by using the NIST database, we find that:

\Delta _fH_{H_2O, liq}=-285.83kJ/mol\\\\\Delta _fH_{SO_2, gas}=-296.84kJ/mol\\\\\Delta _fH_{O_2,gas}=0kJ/mol\\\\\Delta _fH_{H_2S,gas}=-20.50kJ/mol

Thus, we plug in the enthalpies of formation to obtain:

\Delta _rH=2(-285.73kJ/mol)+2(-296.84kJ/mol)-2(-20.50kJ/mol)-3(0kJ/mol)\\\\\Delta _rH=-1124.14kJ/mol

Best regards!

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Explanation:

its A

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