Which of the following graph represents the change in the Potential Energy (PE) of the particles in the system when the substances undergoes the change corresponding to path I?

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: What is the specific heat of a 1,500.00 gram sample of wood that absorbs 67,500 Joules of heat…

A: The given data contains, mass = 1500 g. Heat = 67500 Joules.

Q: If 11.96 kJ of heat is given off when 41.9 g of unknown acid condenses from vapor to liquid, what is…

A: Given data : 11.96KJ  Given mass of unknown acid-41.9g Molar mass of unknown mass 49.15g/mol

Q: For the following thermochemical equation, CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)        ΔH = –890 kJ…

A: Given reaction: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l). ∆H = -890 kJ. So, 890 kJ of heat is released…

Q: which of the following signs on q and w represent a system that is doing work on the surroundings…

A: Given :-  System is doing work on surrounding  System is gaining heat from surrounding  To…

Q: Ethanol (C2H5OH) is used as a base for many fuels. Assume it undergoes complete combustion. How much…

A: The complete combustion reaction for ethanol is given as: C2H5OH(l) + 3O2(g) ----> 2CO2(g) +…

Q: What is the enthalpy change for the following process? N₂(g) + 2H₂(g) → N₂H₂(1) AH = ??? kJ/mol…

A: Here we are required to find the Enthalpy change for the following reaction

Q: An electrical heater is used to supply 210.0 J of energy to a 15.0 g sample of water, originally at…

A: Given:Heat energy (Q) = 210.0 J.Mass of water (m) = 15.0 g.Initial temperature of water = 295…

Q: 3. Given the following thermochemical equations, 4B(s) + 30:(g) → 2B,0;(s) AHO= -2543.8 kJ H2 (g) +…

A: Given reactions are : 1). 4B (s) + 3O2 (g) ---------> 2B2O3 (s), ΔH10 = -2543.8 KJ  2). H2 (g) +…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 643.0 mg sample…

A:

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: 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: Given the following thermochemical data: HNO3(aq)+Ag(s) → AgNO3(aq)+½H2(g)   ΔH = 105.0 kJ…

A:

Q: the laboratory a student finds that it takes 29.3 Joules to increase the temperature of 13.1 grams…

A: Given -> ∆H= 29.3 joule Weight (m) = 13.1 gm T1=20.0°C  T2= 37.9°C

Q: .If a system does 84.0 kJ of work on its surroundings and releases 105 kJ of heat against a constant…

A: Given : Work done on surrounding by system = 84.0 KJ  And heat released = 105 KJ Since heat is being…

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: In an experiment a group gathered the following data: Mass of test tube (g) 21.3 Mass of test…

A: Mass of test tube (g) 21.3 Mass of test tube and metal (g) 52.7 Mass of beaker (g)…

Q: Which of the following processes will increase the potential energy of the system? (You may select…

A: Potential energy of the system is the energy which can be converted to kinetic energy of a system by…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 418.0 mg sample…

A: Given, mass of sample of C2H2Cl2 = 418.0 mg = 0.418 g Initial temperature (Ti) = -5.8°C = (-5.8 +…

Q: 4NH3(g) + O2(g) → 2N2(g) + 6H2O(g)          ΔrH = -1267 kJmol-1  2NO(g) + O­2(g) → 2NO2(g)     ΔrH…

A: For a chemical reaction to be spontaneous, Gibbs free energy, ∆rG should be negative. ∆rG is…

Q: Write out the chemical reaction whose enthalpy is the heat of formation of gaseous methane, CH4.

A: Standard equation of formation is equation represents formation of one mole compound from its…

Q: what is ΔHcond for this substance

A:

Q: If 25.0 kJ of heat are given off when 2.9 g of HCl condenses from vapor to liquid, what is AHcond…

A: Given that: HCl(g) ...> HCl(l) dH = -25.0KJ upon 2.9 g of HCl

Q: The enthalpy of a system can be written as H = U + PV. Show that the enthalpy change AH can express…

A: A question based on chemical thermodynamics that is to be accomplished.

Q: Use the References to access important values if needed for this question. The following…

A: Iron (III) oxide reacts with hydrogen to form iron metal and water. The equation for the balanced…

Q: For the chemical reaction H₂ (g) + F2 (g) → 2 HF (g) AH° = -79.2 kJ/mol. What is the molar enthalpy…

A: In the given question, molar enthalpy of a reaction is given as :-  H2(g) + F2(g) -----> 2HF(g)…

Q: State the law of conservation of energy. How does it relate to energy exchanges between a…

A: For an isolated system, its total energy remains constant. The energy of system will change if it…

Q: Is the total enthalpy (H) of the reactants more than or less than the total enthalpy of the products…

A:

Q: Re-write the equations in the space provided, while applying Hess’s law to determine the enthalpy of…

A: Consider the given overall reaction as; P4O10 (g) + 6 PCl5 (g) → 10 Cl3PO4 (g) Now, consider the…

Q: (b) Study the following thermochemical data very carefully: AH° = 242.3 kJ Cl2(g) → 2Cl(g) I2(g)…

A: The formation of compounds from its atoms in their stable sates at standard pressure and temperature…

Q: A sample of 35.41 g of Cus at 96.73 degrees celcius was added to a calorimeter containing 148.3 g of…

A: Given:…

Q: In endothermic reactions, heat is being absorbed and the internal energy of the system is…

A: Answer:Here:

Q: GIVE AN EXAMPLE OF THESE three types of systems: ~open system- a system that can exchange mass and…

A: Open system- a system that can exchange mass andthe energy with its surroundings Example: A cup of…

Q: Duncan knows that it takes 36400 calcal of energy to heat a pint of water from room temperature to…

A: The amount of energy required to heat a pint of water is 36400 cal. The amount of water taken by…

Q: AH = 66.4 kJ AH = -114.2 kJ N₂(g) +202(g) → 2NO2(g) 2NO(g) + O₂(g) → 2NO₂(g) + - the enthalpy of the…

A:

Q: Under what conditions does the enthalpy change equal the heat of a process

A:

Q: A chemist measures the energy change AH during the following reaction: 2 Fe,O3(s) → 4 FeO(s)+O2(g)…

A: Exothermic reaction: If the energy is released in the reaction. Endothermic reaction: If the energy…

Q: Explain what the equation Q = m•C•ΔT means and how it relates to energy and calorimetry.

A: Explanation of the meaning of the equation Q = mC ΔT :The equation Q = mc ΔT gives the amount of…

Q: The heat capacity of a substance can be obtained by multiplying its mass by its specific heat.…

A: The objective of the question is to determine the units in which the heat capacity of a substance is…

Q: HCl(aq) AH2 = -74.8 kJ (g) → 2 HCI(g) AH3 = -1845.0 kJ → MCI,(aq) AH4 = -300.0 kJ on to determine…

A: According to the question, we have a set of reaction: 2M(s)+6HCl(aq)→2MCl3(aq)+3H₂(g)  ∆ H₁ = -655.0…

Q: 20.0 g of a solid substance X initially at 25.0 °C is heat to its melting point at 65.0 °C. Heat is…

A:

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…

Q: Energy and the First Law of Thermodynamics: We have discussed in the previous discussion the…

A: According to First law of Thermodynamics- ∆U = q + wwhere∆U = total change in internal energy of a…

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.