Thymol has the formula C10H14O and its combustion can be written as: C10H14O(l) + 13 O2(g)...

Question

Question

Thymol has the formula C₁₀H₁₄O and its combustion can be written as:

C₁₀H₁₄O(l) + 13 O₂(g) → 10 CO₂(g) + 7 H₂O(l)

The change in enthalpy of combustion of 1 mole of thymol at 298.15 K is determined to be -5660 kJ at constant pressure.

What is ΔE for this reaction at 298K?

Enter your answer to 4 significant figures in units of kJ. Be sure to include the sign.

Answer 1

Answer #1

The relationship between ∆H and ∆E is given by:

ΔΕ = ΔΗ – pΔV

Which, if pressure is constant and gases can be considered as ideal can be transformed to:

ΔΕ = ΔΗ - RTLηρας

Where ∆n_gas is the change in gaseous moles, which is -3 for the reaction given (10 gaseous moles in proucts and 13 in reagents).

So, we can calculate:

ᎬᎫ AE = -5660kᎫ - 0.008314- , * 2Ꮽ8K * (-3moles) = -5653ᎬᎫ

Answer 2

Similar Homework Help Questions

The complete combustion of acetic acid, HC2H3O2(l) to form H2O(l) and CO2(g) at constant pressure releases...

The complete combustion of acetic acid, HC2H3O2(l) to form H2O(l) and CO2(g) at constant pressure releases 871.7 kJ of heat per mole of HC2H3O2. (a) Write a balanced thermochemical equation for this reaction. (b) Draw an enthalpy diagram for the reaction.
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some...

The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some of the following data to calculate the molar enthalpy of formation of C2H6(g) at 298.15 K 2. Calculate the molar enthalpy of combustion of ethane at 500K Table provided gives values of standard enthalpy of formation values at 298.15 K Substance deltafH (kJ*mol^-1) Cpm (J*K^-1*mol^-1) CO2 (aq) -413.8 N/A CO2 (g) -393.51 37.11 H2O (l) -285.83 75.291 H2O(g) -241.82 33.58 C2H6(g) to be determined...
The thermochemical equation for the combustion of ethanol is: C2H5OH (l) + 3 O2 (g) ->...

The thermochemical equation for the combustion of ethanol is: C2H5OH (l) + 3 O2 (g) -> 2 CO2 (g) + 3 H2O (g) Î”Hrxn = -1360 kJ What is the enthalpy change when 3.50 kg of ethanol react with excess oxygen?

the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The...

the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
The thermochemical equation for the combustion of propane is: C3H8 (g) + 5 O2 (g) ...

The thermochemical equation for the combustion of propane is: C3H8 (g) + 5 O2 (g)  3 CO2 (g) + 4 H2O (l) H = -2220 kJ What is the enthalpy change when 35.0 g of propane react?
Calculate the volume change (in Liters) during the combustion of propane in which ΔE = -3083.67...

Calculate the volume change (in Liters) during the combustion of propane in which ΔE = -3083.67 kJ and ΔH = -3087.12 kJ at a constant pressure of exactly one atm and constant temperature. C3H8(g) + 5 O2(g) ↔ 3 CO2(g) + 4 H2O(l) The product of pressure and volume change should give units of L*atm. It can be shown that 1 L*atm = 101 J.

The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) +...

The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
Consider the combustion of propane: C3H8(g)+O2(g)→CO2(g)+H2O(g) a). Divide all coefficients by the coefficient on propane, so...

Consider the combustion of propane: C3H8(g)+O2(g)→CO2(g)+H2O(g) a). Divide all coefficients by the coefficient on propane, so that you have the reaction for the combustion of 1 mole of propane. Express your answer as a chemical equation. Identify all of the phases in your answer. b). ΔHrxn for the combustion of one mole of propane is −2219kJ. What mass of propane would you need to burn to generate 6.0 MJ of heat? Express your answer to two significant figures and include...
Calculate the standard enthalpy of reaction for the combustion of propane. NOTE: This equation is not...

Calculate the standard enthalpy of reaction for the combustion of propane. NOTE: This equation is not balanced. Round to the nearest whole number. C3H8(g) + O2 --> CO2(g) + H2O(l) kJ/mol Compound Hf (kJ/mole) C3H8(g) -105 CO2(g) -394 H2O(l) -284

Enthalpy changes for the following reactions can be determined experimentally: C2H4(g) + 3 O2(g) → 2...

Enthalpy changes for the following reactions can be determined experimentally: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l) C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) ΔHorxn = -1411.1 kJ/mol-rxn ΔHorxn = -1367.5 kJ/mol-rxn Use the given values to determine the enthalpy change for the reaction: C2H4(g) + H2O(l) → C2H5OH(l) ΔHorxn (answer) = kJ/mol-rxn