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Explain the relationship between Gibb's standard energy change of the reaction and equilibrium constant.
Concept: Chemical Thermodynamics and Energetic >> Equilibrium Constant
Calculate the standard enthalpy of the reaction, 2C(graphite) + 3H2(g) → C2H6(g), ΔH° = ?
From the following ΔH° values
a) `C_2H_6(g) + 7/2 O_2(g) -> 2CO_2(g) + 3H_2 O(l)`. ΔH° = -1560kJ
b) `H_2(g) + 1/2 O_2 (g) -> H_2O(l)` ΔH° = -285.8kJ
c) C(graphite) + O2(g) -> CO2(g). ΔH° = -393.5kJ
Concept: Chemical Thermodynamics and Energetic >> Enthalpy of Bond Dissociation
Write applications of standard molar entropy°.
Concept: Chemical Thermodynamics and Energetic >> Dilution Introduction of Entropy as a State Function
For a certain reaction, ∆H = − 50 kJ and ∆S = − 80 J K-1, at what temperature does the
reaction turn from spontaneous to non-spontaneous?
(A) 6.25 K
(B) 62.5 K
(C) 625 K
(D) 6250 K
Concept: Chemical Thermodynamics and Energetic >> Work, Heat, Energy, Extensive and Intensive Properties
Calculate ∆H° for the following reaction:
2H3BO3(aq) → B2O3(s) + 3H2O(l)
a) H3BO3(aq) → HBO2(aq) + H2O(l) , ∆`H_1^@` = − 0.02 kJ
b) H2B4O7(s) → 2B2O3(s) + H2O(l) , ∆`H_2^@` = 17.3 kJ
c)H2B4O7(s) + H2O(l) → 4HBO2(aq), ∆`H_3^@` = − 11.58 kJ
Concept: Chemical Thermodynamics and Energetic >> Enthalpy of Bond Dissociation
What are the conditions for spontaneous and non-spontaneous reactions in terms of free
energy change?
Concept: Chemical Thermodynamics and Energetic >> Free Energy Change for Spontaneous and Non Spontaneous Processes
What is the action of heat on potassium permanganate?
Concept: Chemical Thermodynamics and Energetic >> Work, Heat, Energy, Extensive and Intensive Properties
Derive the equation : W = - PextAV
Concept: Chemical Thermodynamics and Energetic >> Work, Heat, Energy, Extensive and Intensive Properties
The process in which the value of ΔU = 0 is __
Concept: Chemical Thermodynamics and Energetic >> Types of Systems
Give two uses of the Third law of thermodynamics.
Concept: Chemical Thermodynamics and Energetic >> Second and Third Law of Thermodynamics
Calculate the internal energy at 298K for the formation of one mole of ammonia, if the enthalpy change at constant pressure is – 42.0 kJ mol-1.
(Given: R = 8.314 J K-1 mol-1)
Concept: Chemical Thermodynamics and Energetic >> First Law of Thermodynamics
Define Enthalpy of vaporization
Concept: Chemical Thermodynamics and Energetic >> Internal Energy and Enthalpy
A system absorbs 6 kJ of heat and does 1.5 kJ of work on its surroundings. The change in internal energy is __________.
Concept: Chemical Thermodynamics and Energetic >> Internal Energy and Enthalpy
Write the conditions for maximum work done by the system.
Concept: Chemical Thermodynamics and Energetic >> Chemical Thermodynamics and Energetic
Calculate the work done in the following reaction at 50°C. State whether work is done on the system or by the system.
`"SO"_2("g") + 1/2"O"_(2("g")) rightarrow "SO"_(3("g"))`
Concept: Chemical Thermodynamics and Energetic >> Enthalpy of Bond Dissociation
The standard enthalpy of combustion of formaldehyde Δ0H0 = -571 kJ. How much heat will be evolved in the formation of 22 g of CO2?
Concept: Chemical Thermodynamics and Energetic >> Combustion, Formation, Atomization, Sublimation
5 moles of helium expand isothermally and reversibly from a pressure 40 × 10-5 N m-2 to 4 × 10-5 N m-2 at 300 K. Calculate the work done, change in internal energy and heat absorbed during the expansion. (R = 8.314 J K-1 mol-1).
Concept: Chemical Thermodynamics and Energetic >> Work, Heat, Energy, Extensive and Intensive Properties
Write features of a reversible process.
Concept: Chemical Thermodynamics and Energetic >> Chemical Thermodynamics and Energetic
A substance which shows the highest entropy is ___________.
Concept: Chemical Thermodynamics and Energetic >> Dilution Introduction of Entropy as a State Function
Choose the most correct answer:
Which of the Na following is a buffer solution?
Concept: Buffer Solutions
