Using the provided table of Enthalpies of Formation, determine the enthalpy for the following reaction: 2C6H14(1) + 190,(g) → 12CO,(g) + 14H,O(g) AHf C6H14(1) = -199 kJ/mol AH¡ 02(g) = 0 kJ/mol AH¡ CO2(g) AHf H20(g) A. 8500 kJ/mol = -393 kJ/mol = -242 kJ/mol O B. -7700 kJ/mol OC. -8500 kJ/mol OD.7700 kJ/mol

Using the provided table of Enthalpies of Formation, determine the enthalpy for the following reaction: 2C6H14(1) + 190,(g) → 12CO,(g) + 14H,O(g) AHf C6H14(1) = -199 kJ/mol AH¡ 02(g) = 0 kJ/mol AH¡ CO2(g) AHf H20(g) A. 8500 kJ/mol = -393 kJ/mol = -242 kJ/mol O B. -7700 kJ/mol OC. -8500 kJ/mol OD.7700 kJ/mol

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...

See similar textbooks

Similar questions

A scientist measures the standard enthalpy change for the following reaction to be -876.7 kJ :2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of NH3(g) is kJ/mol.
Using the provided table, determine the enthalpy for the reaction C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AH¡ (kJ/mol) C3H® (g) -108.4 O2 (g) CO2 (g) -393.5 H2O (g) -241.8
Given: 4AICI3(s) + 302(g) → 2Al,O3(s) + 6C12(g); AH=-529.0 kJ determine AH for the following thermochemical equation. Cl,(3) + Al,O;(s) → AICI,(9) + 02(g) O +88.2 kJ O +264.5 kJ O +176.3 kJ O -176.3 kJ O +529.0 kJ
O THERMOCHEMISTRY Using Hess's Law to calculate net reaction enthalpy Lindsay Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO,(g) + 3 H,(g) → CH;OH(1) + H,0(1) AH=-131. kJ In the second step, methanol reacts to form dimethyl ether and water: 2 CH,OH(1) → CH;OCH,(g) + H,0(1) AH=8. kJ Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. II
10. Calculate the standard enthalpy for the reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), given the following data: N2(g) + O2(g) → 2NO(g) ΔHrxn = -43.1 kcal mol-1 N2(g) + 3H2(g) → 2NH3(g) ΔHrxn = -21.9 kcal mol-1 2H2(g) + O2(g) → 2H2O(g) ΔHrxn = -115.6 kcal mol-1
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 SO2(g) + O2(g) → 2 SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are AH; [SO2(g)] = -296.8 kJ/mol AH; [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 2.25 L of SO2(g) is converted to 2.25 L gas behavior. of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal AH= kJ
The enthalpy change for the oxidation of butane, C4H₁0, is measured by calorimetry. C4H10 (g) + 13/2 O2(g) → 4 CO2 (g) +5 H₂O(l) A₂H = -2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = Submit Answer OCT 30 Try Another Version tv kJ/mol S4 I all 9 item attempts remaining Cengage Learning | Cengage Technical Support A MacBook Pro 7 ( O 04
Find the standard change in enthalpy for the following reaction. N₂H4(1) + O₂(g) → 2 NO(g) + 2 H₂O(g) Given the following known reactions: N₂(g) + 2 H₂(g) → N₂H₁ AH = 97.4 kJ/mol N₂(g) + O₂(g) → NO(g) AH = 90.2 kJ/mol H₂(g) + O₂(g) → H₂O(g) AH = -242 kJ/mol Remember you need to include O₂ to get a balanced reaction but its AH = 0 kJ/mol !!
Use the References to access important values if needed for this question. A scientist measures the standard enthalpy change for the following reaction to be -103.2 kJ: 4HCl(g) + O2(g) → 2H₂O(g) + 2Cl₂ (g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(g) is I kJ/mol red Species AH (kJ/mol) H₂O(g) -241.8 Cl₂(g) 0.0 0₂ (9) 0.0
The balanced thermochemical equation for the combustion of exactly one mole of propane is: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O(l) ΔH = -2220 kJ/mol What is the enthalpy change for the reaction: 1.5 CO2 (g) + 2 H2O(l) → 0.5 C3H8 (g) + 2.5 O2 (g) ΔH = ?
When methanol, CH3OH,CH3OH, is burned in the presence of oxygen gas, O2,O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJCH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJ How much methanol, in grams, must be burned to produce 639 kJ639 kJ of heat?
A scientist measures the standard enthalpy change for the following reaction to be -679.7 kJ : 2NH3(g) + 2 02(g)N20(g) + 3 H2O(1) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of N20(g) is |kJ/mol.