QUESTION 11 Which of the following has a standard enthalpy of formation of zero? O3(g) 12(g) Ar(g) Br2(9)

Q: Mercury was once used in thermometers and barometers. When 69.7 J of heat are absorbed by 100.0 g of…

A: Given, Heat absorbed Q = 69.7 J change in temperature ΔT = 29.98 - 25 = 4.98 ℃ Mass m = 100 g

Q: An automobile engine provides 581 Joules of work to push the pistons and generates 2167 Joules of…

A: The relationship between change in internal energy (∆E), heat (q) and work done (W) is given by…

Q: The work done to compress a gas is 93 J. As a result, 38 J of heat is given off to the surroundings.…

A: Work done to compress = Work done on the systemand work done on the system is taken as a positive…

Q: For the reaction, N2(g) + 2 O2(g) ➞ 2 NO2(g) , the enthalpy change is 33.9 kJ/mole of NO2 formed.…

A: Enthalpy is a thermodynamic property which is an extensive additive property we are required to find…

Q: Calculate the standard enthalpy of the reaction, AH° rn. for the thermite reaction: 2Al(s) +…

A: As we know that ΔHoreaction o ​   =∑Products nΔH0t  -∑Reactant nΔH0twhere , ∑Products nΔH0t=Enthalpy…

Q: The heat equation, as given in the introduction, can also be rearranged to calculate the mass or…

A: The specific heat required to raise the temperature of a substance is given as:

Q: 2. When acetone, CH3COCH3, is completely burned to carbon dioxide and liquid water, at 25°C, Delta…

A: The balanced chemical reaction between acetone and oxygen to produce carbon dioxide and liquid water…

Q: In water, The solubility of lead chloride is higher than that of silver chlorides True False

A: True Lead chloride is poorly soluble in water. And it is insoluble in cold water. This is due to the…

Q: Which one of the following has a non-zero value for enthalpy of formation?

A: The enthalpy of formation for N2(g) (nitrogen gas) and Ne(g) (neon gas) and Br2 liquid is indeed…

Q: A student wishes to measure the enthalpy change of the reaction of magnesium oxide solid (MgO, M=…

A:

Q: Use the following information to answer the next question. Given the following data: P4(s) + 6Cl₂(g)…

A: Note: As per the guidelines solution of 1st question has been made and for the expert solution of…

Q: Under Measurements show that the enthalpy of a mixture of gaseous reactants increases by 206. kJ…

A:

Q: Which of the following statement is incorrect? Select all the incorrect statements, wrong choices…

A: Some statements from thermodynamics is given. We need to find the incorrect statement from the given…

Q: A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat…

A: Formula used :  Qbomb = mH2O CpH2O (T2-T1) + Cbomb (T2-T1)

Q: Measurements show that the enthalpy of a mixture of gaseous reactants increases by 391kJ during a…

A: According to the question,The enthalpy of a mixture of gaseous reactants is increased by ΔH = 391…

Q: Measurements show that the energy of a mixture of gaseous reactants decreases by 153. kJ during a…

A: According to the first law of thermodynamics, the total heat change of a system at constant pressure…

Q: When one mole of C6H6C6H6 is burned, 3.27 MJ3.27 MJ of heat is produced. When the heat from burning…

A: The number of moles of C6H6 is 1 mol. The heat released is 3.27 MJ. The weight of C6H6 is 7.87 g.…

Q: which is the correct enthalpy of formation reaction for nitrogen monoxide gas?

A:

Q: A Boy’s calorimeter gave the following results. Volume of gas burned (at standard conditions) =0.01…

A: We are provided with Boy’s calorimeter data.Volume of gas burned (at standard conditions) =0.01…

Q: An electric heater supplies energy to a 25.0 g block of Al. The temperature was originally 22.8 °C…

A:

Q: In the laboratory a student finds that it takes 34.3 Joules to increase the temperature of 13.7…

A:

Q: a You want to determine the value for the enthalpy of formation of CaSO4(s). Ca(s) + S(s) + 2 O2(g)…

A: The objective of this question is to reaction involving calcium (Ca), sulfur (S), oxygen (O), and…

Q: Determine the internal energy change if 718 J of heat are transferred to the system and 437 J of…

A:

Q: Given the following thermochemical equation: 4NH3(g) + 502(g) Calculate the enthalpy change when…

A: Ammonia reacts with oxygen to form nitrogen oxide and water. The equation for the balanced chemical…

Q: Chlorine Tri fluoride is a toxic intensely reactive gas.  It was used in WWII to make incendiary…

A: It is an exothermic reaction having ∆H as negative value and 1196 kJ of heat is evolved.

Q: Measurements show that the energy of a mixture of gaseous reactants decreases by 209. kJ during a…

A: Decrease in Energy of gaseous reactant  = ∆E = -209 kJ Work done = -104 kJ Change in enthalpy of gas…

Q: In the laboratory a student finds that it takes 14.8 Joules to increase the temperature of 10.6…

A: The specific heat (C) of a compound is mathematically expressed as: C=Qm×∆T…

Q: The work done to compress a gas is 70 J.  As a result, 25 J of heat is given off to the…

A: Work done to compress = Work done on the system And work done on the system is taken with a positive…

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.