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oksian1 [2.3K]
3 years ago
12

Acetylene (c2h2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. given δh°f[co2(g)] = –393.5

kj/mol, δh°f[h2o(g)] = –241.8 kj/mol, and δh°f[c2h2(g)] = 226.6 kj/mol, how much energy is released (kj) when 10.5 moles of acetylene is burned?
Chemistry
1 answer:
Brums [2.3K]3 years ago
8 0
Answer is: 13181,7 kJ of energy <span>is released when 10.5 moles of acetylene is burned.
</span>Balanced chemical reaction: C₂H₂ + 5/2O₂ → 2CO₂ + H₂O.
<span>ΔHrxn = sum of ΔHf (products of reaction) - sum of ΔHf (reactants).</span><span>
Or ΔHrxn = ∑ΔHf (products of reaction) - ∑ΔHf (reactants).
ΔHrxn - enthalpy change of chemical reaction.
<span>ΔHf - enthalpy of formation of reactants or products.
</span></span>ΔHrxn = (2·(-393,5) + (-241,8)) - 226,6 · kJ/mol.
ΔHrxn = -1255,4 kJ/mol.
Make proportion: 1 mol (C₂H₂) : -1255,4 kJ = 10,5 mol(C₂H₂) : Q.
Q = 13181,7 kJ.
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Explanation:

Given data:

Volume of KMnO₄ = 255 mL (255/1000 = 0.255 L)

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How many hydrogen atoms are contained in 0.40 mL of water, given that the density of water is 1 g/ml?
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2.676e22 atoms of Hydrogen

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What is the difference in height between the top surface of the glycerin and the top surface of the alcohol? Suppose that the de
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Here is the full question

Glycerin is poured into an open U-shaped tube until the height in both sides is 20 cm. Ethyl alcohol is then poured into one arm until the height of the alcohol column is 10 cm. The two liquids do not mix.

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ΔH ≅ 3.73 cm

Explanation:

The pressure inside a liquid is known as hydrostatic pressure and which is represent by the formula:

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