A scientist measures the standard enthalpy change for the following reaction to be -52.7 k) :C2H4(9) + H20(g)→CH3CH20H(9)Based on this value and the standard enthalples of formation for the other substances, the standard enthalpy of formation of CH3CH2OH(g) IskJ/mol.

Answered: Image /qna-images/answer/92b5f3de-54b9-4865-8945-1919cda743b4.jpg

A scientist measures the standard enthalpy change for the following reaction to be -52.7 k) : C,H4(9) + H20(9) CH3CH»OH(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CH CH2OH(9) is kJ/mol.

A scientist measures the standard enthalpy change for the following reaction to be -52.7 k) : C,H4(9) + H20(9) CH3CH»OH(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CH CH2OH(9) is 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 -2929.4 kJ :2C2H6(g) + 7 O2(g)4CO2(g) + 6 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO2(g) is kJ/mol.
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.
Chemistry A scientist measures the standard enthalpy change for this reaction to be -818.2 kJ/mol:Fe2O3(s) + 2 Al(s)Al2O3(s) + 2 Fe(s)Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of Fe2O3(s) is _____ kJ/mol.
For which one of the following is the enthalpy of the reaction the same as the enthalpy of formation? A) 2 H (g) + Se (s) → H:Se (g) B) KOH (s) → K*(aq) + OH- (aq) C) 2 Fe (s) + 3 Cl2 (g) → 2 FeCl3 (s) D) Ni (s) + ½ O2 (g)- NiO (s)
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
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
A scientist measures the standard enthalpy change for the following reaction to be 216.8 kJ :CH4(g) + H2O(g)3H2(g) + CO(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is kJ/mol.
A scientist measures the standard enthalpy change for the following reaction to be 184.8 kJ:Fe3O4(s) + 4 H2(g) 3Fe(s) + 4 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Fe3O4(s) is kJ/mol.
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 = ?
Hot water heaters often use natural gas (methane) to generate heat. Methane and oxygen react to form carbon monoxide according to the overall equation: 2CH4(g)+3O2(g) = 2CO(g)+4H2O(g) The enthalpy of formation for each compound are as follows: CH4: - 74.6 O2: 0 CO: - 110.5 H2O: - 285.8 Part A: calculate the overall enthalpy change of the reaction. Part B: A typical water heater contains 40.0 gallons of water. After a long vacation, you come home and turn your water heater from "vacation mode" to hot. How many moles of methane must be combusted to heat the water in your water heater from 30.0°C to 48.0°C? The density of water is 3.79 kg/gal, the specific heat capacity of water is 4.182 J/g°C, and the water heater has a heat capacity of 850.0 J/g°C.
A scientist measures the standard enthalpy change for the following reaction to be -912.5 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 H2O(g) is kJ/mol.
Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9) Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9)