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
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The answer is 1.6 atm. I just took the quiz.
Boyle's law gives the relationship between pressure of a gas and volume.
It states that the pressure of a gas is inversely proportional to volume of gas at a constant temperature.
PV = k
where P - pressure , V - volume and k - constant
P1V1 = P2V2
where parameters for the first instance are on the left side of the equation and parameters for the second instance are on the right side of the equation.
1.50 atm x 500.0 mL = P x 150.0 mL
P = 5 atm
applied pressure should be 5 atm to compress the gas.
2Cr”(as)+hc(g)>2Cr(s)+6H*(sa)
