Reaction 3: N2 (9) + 202 (g) → 2NO2(g) AH= +66.4 kJ Complete the table for Reaction 3. Assume the process occurs near room temperature.

Q: Chemical Changes Lab Chemistry Name: Per. Post-laboratory Questions: Answer the following questions…

A: The objective of the question is to find the factors or variables that can change the change the…

Q: Which of the following is not true of spontaneity?     It happens without the addition of external…

A: A spontaneous process occurs automatically without any external force. It is unidirectional

Q: The only absolutely reliable indicator of spontaneity is: a)  enthalpy  b)  entropy  c)  Gibbs free…

A: ∆G = ∆H - T ∆S. Change in Gibbs free energy is equal to change in enthalpy minus the product of…

Q: What is the standard Gibbs free energy of the reaction H2(g) + Br2(g) → 2HB1(g) at 298 K, and is it…

A:

Q: Calculate the value of K, for the reaction 2N₂(g) + O₂(g) 2N₂O(g) at 298.15 K and 1573 K.…

A: Where,Kp = Equilibrium Constant R = Universal gas constant = 8.314 J/mol.KT = Temperature in K ΔG° =…

Q: dye molecules molecules (solvent) (solute) water Explain how diffusion is an Crystal of dye is…

A: The word thermodynamics is composed of two words that are "thermo" which means heat and "dynamics"…

Q: All reactions are endothermic. O True O False

A: All reaction are endothermic, this statement is totally false.

Q: 1/2 Cl2 (g) -><- Cl (g) The reaction Gibbs free energies at various temperatures are given. A)…

A: The Gibbs free energy describe the spontaneity of a reaction, if its value is negative, reaction…

Q: For the reaction 2S02(g) + O2(g)–2SO3(g) AH° = -197.8 kJ and ASº = -187.9 J/K The equilibrium…

A: Given: ∆Ho = -197.8 kJ = -197.8×103 J (Since 1 kJ = 103 J) ∆So = -187.9 J/K Temperature (T) = 271.0…

Q: Consider the reaction: CaCO3(s) ↔ CaO(s) + CO2(g) The reaction enthalpy and entropy are: ΔHo rx =…

A: The expression of thermodynamic equation is shown below: where; T = temperature R = gas constant K…

Q: What is standard temperature and pressure in thermodynamics?

A:

Q: From the data below calculate G for the next reaction (at 298 K) 2CO (g) + O2(g) --&gt; 2CO2(g)

A: The relationship between ΔG for a reaction and ΔH and ΔS is as shown below. ΔG = ΔH - TΔS where ΔG =…

Q: A non-spontaneous reaction is also considered an impossible reaction. True False

A: Given question discusses, how non spontaneity is different from the inaccesibility of a chemical…

Q: In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial…

A: 100ml of H2O is used Initial Temperature = 23oC ∆H = -82.8kJ/mol = 82800J Specific heat = 4.184J/goC…

Q: In going from State A to State B there is an increase in Group of answer choices entropy none of the…

A: The correct answer is given below

Q: What is the standard free energy change for the ionization of H2O2 acid, if its Ka is 2.40e-12

A: ∆G=-RT lnK     = -(8.314*298) ln2.4*10-12     =-(2477.57)*(-29.058)     = 66.326 KJ

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.    

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.