The standard enthalpy of formation of liquid hexane is ∆?? ⊖ = −196.0 ????? −1 .
(i) Knowing that the standard enthalpy of vaporization of hexane is ∆?? ⊖ = +28.9 ????? −1 , estimate the enthalpy of formation of gaseous hexane. [6 marks]
(ii) Knowing that the standard enthalpy of formation of liquid cyclohexane is ∆?? ⊖ = −156.0 ????? −1 , estimate the standard enthalpy of cyclization of liquid hexane. Is the reaction endothermic or exothermic?
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The standard enthalpy of formation of liquid hexane is ∆?? ⊖ = −196.0 ????? −1 ....
The compound 1-propanol,
C3H8O, is a good fuel. It is
a liquid at ordinary temperatures. When the liquid is burned, the
reaction involved is
2 C3H8O(ℓ) + 9
O2(g)6
CO2(g) + 8
H2O(g)
The standard enthalpy of formation of liquid 1-propanol at 25 °C is
-302.6 kJ mol-1; other relevant
enthalpy of formation values in kJ mol-1 are:
C3H8O(g) =
-255.1 ; CO2(g) =
-393.5 ; H2O(g) =
-241.8
(a) Calculate the enthalpy change in the burning of
3.000 mol...
The compound 1-pentanol, C5H12O, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is 2 C5H12O(ℓ) + 15 O2(g)10 CO2(g) + 12 H2O(g) The standard enthalpy of formation of liquid 1-pentanol at 25 °C is -351.6 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are: C5H12O(g) = -294.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 (a) Calculate the enthalpy change in the burning of 5.000 mol...
The compound heptane, C7H16, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is C7H16(ℓ) + 11 O2(g)7 CO2(g) + 8 H2O(g) The standard enthalpy of formation of liquid heptane at 25 °C is -224.2 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are: C7H16(g) = -187.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 (a) Calculate the enthalpy change in the burning of 2.000 mol liquid...
(a) Explain the difference between the enthalpy of formation of liquid and gaseous water,-286 and - 242 kJ/mol, respectively, at 298 K. b) Explain why the enthalpy of vaporization of water at 100 oC (40.7 kJ/mol) is lower than at 25 oC (44 kJ/mol)
Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/mol
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
Question 5 (1 point) The reaction of aluminum with oxygen is exothermic. The enthalpy of formation for aluminum oxide is - 1676 kJ/mol. How much heat will the combustion of 4.50 g of aluminum produce, in kJ? Include the proper sign for an exothermic or endothermic reaction.
The standard enthalpy of formation of NH_2(g) id -46 KJ mol^-1.The standard enthalpy of formation of H_2O(g) is -242 KJ middot mol^-1. The enthalpy of reaction is 906 kl. The standard enthalpy of formation of NO(g)is a. -754.5 kJ middot mol^-1 b. -362 kJ middot mol^-1 c. -196.5 kJ middot mol^-1 d. -90.5 k middot J-mol^-1 e. +90.5 kJ middot mol^- 1 f. +182.5 kJ middot mol^-1 g.+317 kJ middot mol^-1 h. +362 kJ middot mol^-1 i. +409 kJ middot...
Enthalpy of Formation
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A scientist measures the standard enthalpy change for the following reaction to be 591.0 kJ : 2H2O(1)—>2H2(g) + O2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(l) is kJ/mol. A scientist measures the standard enthalpy change for the following reaction to be -2903.4 kJ: 2C2H6(g) + 7 O2(g)—>4CO2(g) + 6 H2O(g) Based on this value and the standard...
Question 7 1 pts What is the meaning of the negative sign in the standard enthalpy of combustion of butane (-2877 kJ mol-1) Endothermic reaction Exothermic reaction Enthalpy Thermodynamic reaction