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tester [92]
2 years ago
14

Based on the bond energies for the reaction below, what is the enthalpy of the reaction?HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O

(g)
Chemistry
1 answer:
Anuta_ua [19.1K]2 years ago
8 0

Answer:

1219.5 kj/mol

Explanation:

To reach this result, you must use the formula:

ΔHºrxn = Σn * (BE reactant) - Σn * (BE product)

ΔHºrxn = [1 * (BE C = C) + 2 * (BE C-H) + 5/2 * (BE O = O)] - [4 * (BE C = O) + 2 * (BE O-H).

The BE values are:

BE C = C: 839 kj / mol

BE C-H: 413 Kj / mol

BE O = O: 495 kj / mol

BE C = O = 799 Kj / mol

BE O-H = 463 kj / mol

Now you must replace the values in the above equation, the result of which will be:

ΔHºrxn = [1 * 839 + 2 * (413) + 5/2 * (495)] - [4 * (799) + 2 * (463) = 1219.5 kj/mol

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The force that holds protons and neutrons together is too strong to overcome.

<h3>Explanation</h3>

Consider the location of the particles in an atom.

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Protons carry positive charges and repel each other. The nucleus will break apart without the strong force that holds the protons and neutrons together. This force is much stronger than the attraction between the nucleus and the electrons. X-rays are energetic enough for removing electrons from an atom. However, you'll need a collider to remove protons from a stable nucleus. You could well have ionized the atom with all that energy.

Also, changing the number of protons per nucleus will convert the halogen atom to an atom of a different element. Rather than making the halogen negative, removing a proton will convert the halogen atom to the negative ion of a different element.

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2 years ago
A sample of an ideal gas occupies 2.78 x 10^3 mL at 25°C and 760 mm Hg.
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Answer: It will occupy 4.45\times 10^3ml at the same temperature and 475 mm Hg.

Explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

P\propto \frac{1}{V}     (At constant temperature and number of moles)

P_1V_1=P_2V_2    (At constant temperature and number of moles)

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P_1 = initial pressure of gas = 760 mm Hg

P_2 = final pressure of gas = 475 mm Hg

V_1 = initial volume of gas = 2.78\times 10^3ml

V_2  = final volume of gas = ?

Putting in the values:

760mm Hg\times 2.78\times 10^3ml=475 mm Hg\times V_2

V_2=4.45\times 10^3ml

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<h3>Answer:</h3>

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