The combustion of isooctane (C₈H₁₈) is written below:
2 C₈H₁₈ (l) + 25 O₂ (g) → 16 CO₂ (g) + 18 H₂O (l)
The formula for heat of combustion is:
ΔHc = (∑Stoichiometric coefficient×ΔHf of products) - (∑Stoichiometric coefficient×ΔHf of reactants), where ΔHf is heat of formation.
ΔHf of isooctane = -259.2 kJ/mol
ΔHf of O₂ = 0 kJ/mol
ΔHf of CO₂ = -393.5 kJ/mol
ΔHf of H₂O = <span>-285.8 kJ/mol
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ΔHc = [(16 mol×-393.5 kJ/mol )+(18 mol×-285.8 kJ/mol)] - [(2 mol×-259.2 kJ/mol) + (25 mol*0 kJ/mol)]
ΔHc = -10,922 kJ
Answer:
It doesn't disappear.
Explanation:
Water vapor does not disappear. It loses its solid form because it is warm enough, and thus becomes an invisible gas.
A combustion reaction is when a fuel, usually a hydrocarbon, reacts with excess oxygen to form carbon dioxide gas and water vapor.
Answer:
B) 10.1 L
Explanation:
Hello,
In this case, for the given chemical reaction which should be corrected as shown below:
Since 45.0g of calcium carbonate are used, the produced moles of carbon dioxide, via stoichiometry, are found to be:
Finally, since STP conditions are referred to a temperature of 273.15K and 1 atm, the volume, by using the ideal gas equation result:
So the answer is B) 10.1 L.
Best regards.
Answer:
Explanation:
The answer is (4) 4.0 mol. This is a stoichiometry problem. You start with 2.0 mol of C2H6 and obtain the moles of C by multiplying 2.0 by the mole ratio, in this case 2. 2.0*2=4.0mol.