Calculate AHrxn at a. 298K and b. 478K for the reaction, C(graphite) + H₂O(g) → CO(g) + H₂(g) given: CO(g) H₂O(g) H₂(g) C(graphite) AH₁ -110.53kJ/mol -241.82 0 0 Cpm (assume C's are constant for the given T range) 29.14 J/kmol 33.58 J/kmol 28.82 J/Kmol 8.53 J/Kmol

Q: Given the following reaction C(s)+ 800₂(g) → 57 CO₂(g)+ 52H,00) AH comb 35100 kJ = mol determine the…

A: We need to find the amount of heat absorbed or released when 454 g of C57H104O6​ is burned in the…

Q: Using values from Appendix C of your textbook, calculate the value of Ho, So, and Go for each of the…

A: The given reaction is: 3 NO(g) ------> NO2(g) + N2O(g)

Q: Find AHrxn (kJ/mol) for the reaction 2Al(s) + Fe203(s) → Al203(s) + 2Fe(s), given the reactions…

A: The reactions given are,

Q: Answer the following questions about the chemical reaction shown below. Thermo data is provided.…

A: Given  4NO2 (g). + O2(g) ---> 2N2O5(g)  Molecule ∆Hf0kJ/mol N2O5 13.3 NO2 33.2 O2 0

Q: How much energy is required to heat 85.5 g of acetone, (CH3)2CO, from -162°C to -48°C? The following…

A: Given data is Mass of acetone = 85.5 g of acetone  Initial temperature of acetone=  -162°C Final…

Q: Metal Specific Heat Aluminum 0.897 J/(g°C) Magnesium 1.02 J/(g°C) Tungsten 0.134 J/(g°C) Silver…

A: Given Mass of aluminium = 43.6 g initial temperature of aluminium = 82.4°C initial temperature of…

Q: Enormous amounts of lime (CaO) are used in steel industry blast furnaces to remove impurities from…

A: The reaction is: Kp = 1/Partial pressure. Then,

Q: Answer the following questions based on the given information at 25.0°C. 2N2H«(g) + 2NO2(g) → 3N2(g)…

A: Formula used :- ∆G° = ∆H° - T∆S°

Q: Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction is 5.82  × 10–4,…

A:

Q: The AHxn for the combustion of 5.0 moles of butane (C4H10) is closest to = -5754 kJ/mol 2C4H10(9) +…

A: Combustion of hydrocarbon is the process of burning hydrocarbons in presence of oxygen. On…

Q: In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon…

A:

Q: determine the enthalpy change for reaction 1. (1)         Mg(s) + 1/2O2(g) → MgO(s)…

A: Hess' law of constant heat summation: The Hess law states that the change of enthalpy in a chemical…

Q: The reaction of iron(s) with chlorine(g) to form iron(III) chloride proceeds as follows: 2Fe(s)+…

A: The iron metal reacts with the chlorine gas to form iron(III) chloride. The equation for the…

Q: Consider the reaction: NO (g)+1/2 02 (8) --> NO2 (8) Given the following data: So (NO)=203.89J/mol K…

A:

Q: Which of the following processes would you predict to have the most favorable ΔSº?     CH3OH(g)  →…

A: Entropy  It is defined as the randomness present in the system. If the randomness is more then…

Q: O and NO must be converted to less harmful gases through the following reaction: CO(g) + NO(g)…

A:

Q: A bomb calorimeter (C = 39.97 kJ/⁰C) is used for the controlled combustion of some ethanol. The…

A: Given:Specific heat of calorimeter C = 39.97 kJ/⁰CInitial temperature = 20.0⁰CFinal temperature =…

Q: Hess's law: Given the following at 25oC and 1.00 atm: 1)  SO3 (g)     +     H2O (l)    →     H2SO4…

A: Given 1)  SO3 (g)  + H2O (l) →  H2SO4 (l)         ΔHo = -133 kJ 2)  Pb (s) + PbO2 (s) + 2H2SO4 (l)…

Q: Calculate the heat of decomposition for this process at constant pressure and 25°C. (10 points)…

A:

Q: The heat capacity of a bomb calorimeter is found to be 5.68 kJ °C-1. When a 1.652 g sample of…

A: mole = massmolar mass

Q: The combustion reaction for Compound X is given. X(s) + 6 O2(g)→5 CO2(g) + 6 H2O(ℓ)∆H◦for this…

A:

Q: How logn would it take to convert 100 g Na(s) at 20oC to sodium vapor at 1000oC if heating rate at a…

A: To calculate: time taken to convert 100 g Na(s) at 20oC to sodium vapor at 1000oC if heating rate at…

Q: Urea, CO(NH2)2 is slowly converted to ammonia (NH3) at 25.0 °C according to the following reaction.…

A: The reaction for decomposition of urea is,CO(NH2)2 (aq) + H2O (l) → CO2 (aq) + NH3 (aq)Heat of the…

Q: Consider the following reaction at 25 °C: 3 Ni(s) + N₂(g) + 3 H₂O(g) → 3 NiO(s) + 2 NH3(g) If AG =…

A: To calculate ∆G, we use the formula :  ∆G = ∆G° + RTln(Q)  So, we first need to calculate Q (…

Q: Adding nitric acid to water is quite exothermic. Calculate the temperature change (AT) when 100.0 mL…

A: Assuming the density of concentrated HNO3 is same as that of water and its addition doesn't add a…

Q: A 112.1 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C.…

A: In the given process the substance is cooled, hence the heat is released in this process.

Q: For the reaction 2HBr(g) + Cl2(g)2HCl(g) + Br2(g) H° = -81.1 kJ and S° = -1.20 J/K G° would be…

A: 2HBr(g) + Cl2(g) <====> 2HCl(g) + Br2(g) ∆H° = -81.1 kJ ∆H° = -81100 J             { 1kJ =…

Q: 3. At 37°C, the combustion of methane, CH4, has a AH of -2000 kJ. What is the AS surroundings of…

A:

Q: Nitrogen dioxide, NO2, an air pollutant, dissolves in rainwater to form a dilute solution of nitric…

A:

Q: determine the enthalpy change for reaction 1. (1)         Mg(s) + 1/2O2(g) → MgO(s)…

A: The reactions given are, (1) Mg(s) + 1/2O2(g) → MgO(s)                                          ∆H1…

Q: Diborane (B2H6) is a propellant.  The combustion reaction of diborane is as follows: B2H6(s) +…

A:

Q: Consider the following reaction at 25 °C: 5 SO(g) + 2 NH3(g) → 2 NO(g) + 5 SO₂(g) + 3 H₂O(g) Given…

A: Since, Entropy is a thermodynamic quantity. It measure the randomness. If randomness is more then…

Q: The combustion of what volume of ethane (C2H6), measured at 23.0°C and 752 mmHg, would be required…

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: A mixture of 7.8 mol of H₂ (g) and 3.9 mol of O₂ (g) is placed in a sealed evacuated container made…

A: The hydrogen (H2) and oxygen (O2) can react with each other to form water under suitable conditions.…

Q: Calculate the Gºrxn using the following information. AHᵒf (kJ/mol) S°(J/mol*K) 4 HNO3(g) +5 N₂H4(l)…

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.