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puteri [66]
2 years ago
12

Using the bond energy values in the previous question, which molecule

Chemistry
1 answer:
oksano4ka [1.4K]2 years ago
5 0

Hydrogen molecule is a molecule that releases the most energy when forming its bonds as compared to other molecules.

<h3>What bond needs more energy?</h3>

We know that H-H bond energy is 432 kJ mol-1, CI - CI bond energy is 239kJ mol-1 and Br-Br bond energy is 193 kJ mol-1 so from this data we can conclude that more energy is required to break the bond between hydrogen atom.

Learn more about bond here: brainly.com/question/25596583

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At absolute zero the kinetic energy of the substance will be 0
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Carbon, oxygen And nitrogen all types of
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molecules or protein molecules

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In order to ice to melt it must absorb heat This makes it an blank process.
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Answer: A. Endothermic

Explanation:

In an endothermic reaction, heat is sucked in from the surrounding area by the reactants so that they may use it to react and form new products. This will therefore reduce the temperature in the said surrounding by the amount that the reaction needed.

This is what ice does when it melts. It sucks in the heat surrounding the area and then melts but leaves the area colder. For instance, putting ice in water ensures that the ice melts but because it sucked in the heat from the water to do so, the water gets colder as a result.

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3 years ago
What is the basis of a metallic bond?
Luba_88 [7]
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The entropy of a system at 337 K increases by 221.7 J/mol•K. The free energy value is found to be –717.5 kJ/mol. Calculate the c
OlgaM077 [116]

<u>Answer:</u> The change in enthalpy for the given system is -642.8 kJ/mol

<u>Explanation:</u>

To calculate the change in enthalpy for given Gibbs free energy, we use the equation:

\Delta G=\Delta H-T\Delta S

where,

\Delta G = Gibbs free energy = -717.5 kJ/mol = -717500 J/mol    (Conversion factor: 1 kJ = 1000 J)

\Delta H = change in enthalpy = ?

T = temperature = 337 K

\Delta S = change in entropy = 221.7 J/mol.K

Putting values in above equation, we get:

-717500J/mol=\Delta H-(337K\times 221.7J/mol.K)\\\\\Delta H=-642787J/mol=-642.8kJ/mol

Hence, the change in enthalpy for the given system is -642.8 kJ/mol

4 0
3 years ago
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