Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide. 2 C8H18 (l) + 25 O2(g) → 16 CO2 (g) + 18 H₂O(l) A, H = -10, 922 kJ/mol-rxn What is the enthalpy change if you burn 6.00 L of isooctane (d = 0.69 g/mL)? Enthalpy change kJ

Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide. 2 C8H18 (l) + 25 O2(g) → 16 CO2 (g) + 18 H₂O(l) A, H = -10, 922 kJ/mol-rxn What is the enthalpy change if you burn 6.00 L of isooctane (d = 0.69 g/mL)? Enthalpy change kJ

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The combustion of 1.839 g of glucose (C6H12O6) in a bomb calorimeter (Ccal = 4.60 kJ/℃) results in a temperature increase of 6.23℃. What is the molar enthalpy of combustion (ΔHM) of glucose in kJ/mol?
The enthalpy (or heat) of combustion of acetone, (CH3)2CO, is - 1657.8 kJ. The reaction is (CH3)2CO (1) +4 0₂ (g) →3 CO₂(g) + 3 H₂O (g). Given the values of AH-393.5 kJ/mol for CO₂ (g) and AH-241.8 kJ/mol for H₂O(g), the calculated value of AH; for acetone O equals - 3563.7 kJ/mol O equals - 1022.5 kJ/mol O equals-248.1 kJ/mol O equals 1202.7 kJ/mol
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Using the data given, calculate the standard enthalpy of combustion of C₂H₆ in kJ/mol? Thermochemical Data H₂(g) + 1/2O₂(g) → H₂O(l) ΔH°= –286 kJ C₂H₄(g) + H₂(g) → C₂H₅(g) ΔH°= –137 kJ C₂H₄(g) + 3O₂(g) → 2CO₂(g) + 2H₂O(l) ΔH°= –1412 kJ A) –1275 kJ B) –1548 kJ C) –31561 kJ D) +1834 kJ
Given that enthalpy of formation of the several compounds: C(s)+O2(g)>CO2(g);AH=-393.5kJ S(s)+O2(g)→SO2(g);AH=-296.8kJ C(s)+2S(s)→CS2(1);AH=+87.9 kJ Determine the enthalpy of combustion reaction of carbon disulfide!
Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide. 2 C3H13 (2) + 25 02 (g) → 16 CO2(g) + 18 H2O(£) A,H° = -10,922 kJ/mol-rxn What is the enthalpy change if you burn 7.50 L of isooctane (d = 0.69 g/mL)? Enthalpy change |kJ =
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