Determine the product of the ff. rxn steps 1. KMNO4/heat 2. NH3 3.ОН- 4. Brz.КОН А. В. С. D. .CO2 NH2 `NH2 `NH2 `NH2 -NH2

Q: It states that individual molecules may gain or lose energy as a result of collisions. In a…

A: The law of conservation of energy states that-  Energy can neither be created nor be destroyed. It…

Q: Given the following data, calculate the normal boiling point for formic acid (HCOOH).…

A: Given that :   ΔHf°(kJ/mol) S°(J/mol K) HCOOH(l) -410. 130.0 HCOOH(g) -363 250.8…

Q: 3. Use the data below to calculate AH°xn for the reaction MgO) + CO2e MGCO3(6). AH°F MgO) = -602 kJ…

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Q: a) Calculate the AH far the fellowiveg reaction usivng Heas' Law: i) CS 2+2H2O +COz+ 2H2S Gilen…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Consider the problem below: (Equation 1) 4 AICI3 (5) + 2 Al(s) + 3 Cl2(g) - 3 Al,Cla(g) AH = -1051…

A: 6Al(s) + 9Cl2(g) ---> 3Al2Cl6(g)

Q: Please show how to solve

A: The activation energy can be calculated using the formula:

Q: Use the data below to calculate AG°rxn for the reaction: A+ 2B > 2C+ 2D Data: A+2B → 4C AG° rxn…

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Q: Calculate ΔH for the reaction: C6H6(l)   +   O2(g) à   6CO2(g)   +   3H2O(l) given the following…

A: Given that: To find: ∆H for the given reaction =?

Q: b. ∆H0sys

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Q: Calculate Kₚ for each of the following equilibria:

A: (a) Given:

Q: Calculate ΔH for the reactionC1s2 + H2O1g2¡ CO1g2 + H21g2given the following thermochemical…

A: From the given equations, it is clear equation (4) can be obtained by adding equation (1), reverse…

Q: Given the data below, H°rxn for the reaction 2SO2(g)+O2(g) —> 2SO3(g) is ______ kJ ΔH°f(SO2(g))=-297…

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Q: A temperature of -25°C is equivalent to K. Sho BIU E E 1 C-274.15=274.15K

A: Given , Temperature = -25°C  In kelvin = ?

Q: Consider the problem below: (Equation 1) 2 H2O(l) ---> 2 H2(g) + O2(g) ΔH = 571.6 kJ (Equation 2)…

A: Total amount of heat content of a thermodynamic system is known as enthalpy of reaction,  it is sum…

Q: Calculate A Gº for H₂O(g) + O₂(g) H2(g) + O2(g) = H 20 2(g) 2H 2(g) + O2(g) = 2H 20(g) a. 501 kJ b.…

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Q: Hn Idul gas undergoes W, and A Ŭ bc The hat absorbed by gas, work done loy sas, and change m…

A: Given: The process is isothermal expansion process.

Q: several equations

A:

Q: From the following reaction and data, find     (a) S o     of SOCl2     (b) T at which…

A: (a)The quantity that predicts the spontaneity of a process is called Gibbs free energy. The…

Q: Calculate the value of ?p for the equation   C(s)+CO2(g)↽−−⇀2CO(g)?p=? given that at a certain…

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Q: If AH°, of H,0L is -285.8 KJ/mol and AH° of H,O the AH°, of evaporation of H,O in ( KJ/mol) iİs : is…

A: Since you have posted multiple unrelated questions, we are entitled to answer the first only. Given:…

Q: Acetylene burns in air according to the following equation:   C2H2(g) + 5/2 O2(g) →2 CO2(g) +…

A: The standard free energy of formation refers to the energy change that occurs when a compound is…

Q: Calculate ΔHΔH for the reaction B2H6 (g) +  6 Cl2 (g) ⟶⟶ 2 BCl3 (g) + 6 HCl (g) from the following…

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Q: paper substance c. nectar juice solute d. UV energy e. cotton fabric f. yellow light energy g.…

A: Moles are calculated for the chemical substances by relating the number of roles with the number of…

Q: equilibaium congtant K. Cateutate a occueig at temp. of e6c, with oG of -2.7 KJ/mol 2 R=8.314…

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Q: u.co Consider the following reaction at 25 °C: Ba(OH)2 8 H20(s) + 2 NHẠCI(s) → BaCl2(s) + 2 NH3(g) +…

A: The standard entropy change of a chemical reaction is given by the sum of standard entropies of the…

Q: Consider the problem below: (Equation 1) H2(g) + 1/2 O2(g) ---> H2OU) AH = -285.8 kJ/mol (Equation…

A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…

Q: Calculate the value of ?p for the equation   C(s)+CO2(g)↽−−⇀2CO(g)?p=?     given that at a…

A: The equilibrium constant for reaction Kp1 = 3.37 The equilibrium constant for reaction Kp2 = 0.657…

Q: Compound Δ?∘f (kJ/mol)Δ⁢Gf∘ (kJ/mol) A +387.7+387.7 B +600.4+600.4 C +402.0+402.0 Use the data given…

A: Ans given below

Q: H2SiCl2 + H2O −→ H8Si4O4 + HCl Rewrite the Equation and show work

A: The given reaction is  H2SiCl2 + H2O ——> H8Si4O4 + HCl We are to re-write the given balanced…

Q: Determine AHjattice for KBr if the AHsolution (KBr) = +19.9 kJ/mol and the AHnydration (KBr) =…

A: Lattice energy is the amount of energy required to break one mole of crystal lattice of an ionic…

Q: For the reaction ABC + D ⇌ AB + CD  ΔH at 0 for rxn = −70 kJ/mol and Ea(fwd) = 345 kJ/mol. Assuming…

A: The enthalpy of the reaction can be expressed as follows-

Q: Using the bond energies below (kJ/mol), calculate the estimated AH of the reaction pictured below…

A: To calculate the value of ∆H using bond energies , we would use a formula .

Q: Calculate   ∆Horxn    for the following reaction         2H2O2(l)     2H2O(l) + O2(g) given that…

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Q: Rewrite the Equations and show work H2SiCl2 + H2O −→ H8Si4O4 + HCl

A: We can rewrite the given equation by balancing it.  We need to balance the equation for the law of…

Q: Exit Ticket Using your knowledge of Boltzmann Distributions: Label the graph by Prob temperatures…

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Q: Calculate ΔH for this reaction N2H4 (l) + O2 (g) → N2 (g) + 2H2O (l) given the following data:…

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Q: The heat of combustion of liquid octane (C3H130) to carbon dioxide in liquid water at 298 K is…

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Q: Calculate for kredox the for this given equation Pb(s) → Pb+2 + 2e-

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Q: he heat capacities of nitrogen gas at constant volumes were measured at the ollowing temperatures…

A: a) Step 1:Make a new Excel file and put the datas as shown T(K) CV(J .mol-1.K-1) 300 20.8 400…

Q: Using the table of thermodynamic data provided, for the reaction below: SiH4(g) + 8HNO3(g) → SiO2(s)…

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Q: Calculate S when 0.0385 mol of an ideal gas (Cv,m = 1.5R) at 20.0oC and 1.30 atm expand to 0.900…

A: Temperature can be converted from degree celsius to kelvin by the expression: T1K=20+273.15=293.15…

Q: Calculate ∆S° for C₃H₄(g) + 2 H₂(g) → C₃H₈(g).     C₃H₄=266.9 S°(J/mol*K) H₂ = 130.6 S°(J/mol*K)…

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Q: - Consider the problem below: (Equation 1) 2 HF(g) ---> H2(g) + F2(g) ΔH = 537 kJ/mol (Equation 2)…

A: The given equations is as follows: Equation 1:   2HF(g)  →  H2(g) + F2(g)      ∆H1=537 kJ/mol…

Q: You were tasked to do a simple calorimetry experiment to determine the enthalpy of reaction of HNO3…

A: Given: Concentration of HCl = 1.00 M Concentration of NaOH = 1.00 M Volume of NaOH solution added =…

Q: Calculate the EA of F(g), in kJ/mole, given the following IE1 + IE, Sr(g) = +1580 kJ/mole…

A: IE1 + IE2 Sr(g) = +1580 kJ/mole ∆H(sublimation) Sr(s) = +144 kJ/mole ∆H(dissociation) F2 = +79…

Q: Consider the problem below: (Equation 1) H2(g) + 1/2 O2(g) H20(1) AH = -285.8 kJ/mol ---> %3D…

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Q: 1. Initially 0.1 mol of methane is at 1 bar pressure and 80°C. The gas behaves ideally the value of2…

A: Solution -

Q: Use the data below to calculate ΔHf for benzene, C6H6(l), at 25oC and 1 atm.           2C6H6(l)   +…

A: Given reaction,    2C6H6(l)   +   15O2(g)   ®   12CO2(g)   +   6H2O(l)   ΔH = -6535 kJ

Q: Cyclopentene, C,H, is a colorless liquid at room temperature that is used in the synthesis of…

A: An equation which shows the rate of a reaction in terms of the molar concentrations of the reactants…

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.