Given the standard enthalpy changes for the following two reactions: (1) Ni(s) + Cl₂(g)→→→→→→→NiCl₂(s) AH° = -305.3 kJ (2) Pb(s) + Cl₂(g) →→→→PbCl₂(s) ΔΗ° = .359.4 kJ what is the standard enthalpy change for the reaction: (3) Ni(s) + PbCl₂(S) NICl₂(s) + Pb(s) →NiCl₂(s) + Pb(s) AH° = ? kj

Q: In a constant‑pressure calorimeter, 65.0 mL of 0.350 M Ba(OH)2 was added to 65.0 mL of 0.700 M HCl.…

A: Given:65.0 mL of 0.350 M Ba(OH)265.0 mL of 0.700 M HCl.Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O

Q: Consider these reactions, where M represents a generic metal. 2 M(s) + 6 HCI(aq) → 2 MCI, (aq) + 3…

A: Hess's law states the enthalpy change for the overall reaction is the sum of the enthalpies of…

Q: Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(g) C4H10(g) AH…

A: In Hess's law, the enthalpy of the resultant reaction remains the same if this reaction takes place…

Q: When a 8.00 g sample of KCI is dissolved in water in a calorimeter that has a total heat capacity of…

A: Given : Mass of KCl dissolved = 8 g Total heat capacity of calorimeter = 6.15 KJ/K And change in…

Q: Consider these reactions: Reaction 1: H2 (g) + Cl2 (g) → 2HC1(g) AH = -184.6 kJ Reaction 2: 20F2 (g)…

A: -> If ∆H =+ve => reaction is endothermic reaction. -> if ∆H = -ve => reaction is…

Q: In a constant‑pressure calorimeter, 65.0 mL of 0.340 M Ba(OH)2 was added to 65.0 mL of 0.680 M HCl.…

A:

Q: From the enthalpies of reaction: 2 C(s) + O2(g) → 2 CO(g) ΔH =…

A:

Q: Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction:…

A:

Q: The enthalpy change for the reaction of hydrogen gas with fluorine gas to produce hydrogen fluoride…

A:

Q: Use this information 2H(aq) → H(g) ΔH = -305.6 kJ/mol Zn(s) + 2Cl(aq) → ZnCl(aq) ΔH = -451.1 kJ/mol…

A:

Q: In a coffee cup calorimeter, a student places 0.470 g of calcium, followed by addition of 50.0 mL of…

A: Given, maas of Ca= 0.470 g  As HCl have properties like water so density= 1g/ml  So mass od 50 ml…

Q: During an experiment, a student adds 1.23 g CaO to 200.0 mL of 0.500 M HCI. The student observes a…

A:

Q: A chemist measures the enthalpy change AH during the following reaction: 2 Na(s) + Cl,(g)–→2 NaCl(s)…

A: Given: ∆H for the reaction 2Na(s) + Cl2(g)----> 2NaCl(s) is -822 kJ

Q: Given the standard reaction enthalpies for these two reactions: (1) N2(g) + 20,(g) →N2O4(g) A,H° =…

A: Given  N2(g) +  2O2(g)   →  N2O4(g)                ∆rH°  =  9.2 KJ/mol                 [ Equation 1…

Q: How many total species there are in sodium citrate

A: Sodium citrate is the sodium salt of citrate ion.

Q: During the calculation process, how must the following reaction and its ΔH°rxn be manipulated?…

A:

Q: When a 3.76 g sample of solid ammonium nitrate dissolves in 60.0 g of water in a Styrofoam-cup…

A: Interpretation-  To determine  ΔH (in kJ/mol NH4NO3) for the solution when 3.76 g sample of solid…

Q: In a constant‑pressure calorimeter, 60.0 mL of 0.310 M Ba(OH)2 was added to 60.0 mL of 0.620 M HCl.…

A: Interpretation -  To determine the heat ( Δ) for this reaction (per mole H2O produced) when in a…

Q: Calculate the enthalpy of the reaction 4B(s) + 302(g)–+2B2O3(s) given the following pertinent…

A: The given reactions are as follows, 1. B2O3(s) +3H2O(g) → 3O2(g) + B2H6(g)       ∆HAo = +2035 kJ2.…

Q: Consider the reaction: When a 10.0-g sample of ethyl alcohol (molar mass = 46.07 g/mol) is…

A: The given reaction is : C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l)        ∆H=-1.37×103 kJ

Q: Given the standard enthalpy changes for the following two reactions: (1) Sn(s) + Cl₂(g) → SnCl₂ (s)…

A:

Q: When a 2.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity…

A: The molar heat is the quantity of heat required by one mole of a substance to raise its temperature…

Q: During an experiment, a student adds 1.23 g Ca0 to 200.0 mL of 0.500 M HCI. The student observes a…

A: Generally the heat released in the reaction is absorbed by the solution and raises the temperature…

Q: Given the standard enthalpy changes for the following two reactions: (1) 2Pb(s) + O₂(g) → 2PbO(s)…

A: Recall the given reactions,                          1 2 Pb s  +  O2 g  →  2 PbO s…

Q: The standard enthalpy change for the following reaction is -479 kJ at 298 K.

A: 1) Heat energy change at constant temperature and pressure is called enthalpy change (or) Heat of a…

Q: Consider the dissolution of ammonium nitrate according to the following equation: NH,NO3(s) → NH,…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3 sub-parts. Please resubmit the…

Q: Given the standard enthalpy changes for the following two reactions: (1) 2C(s) + 2H₂(g) → C₂H4 (9)…

A: As per the Bartleby policy, we will answer only the first question. Please repost the second…

Q: Given the standard enthalpy changes for the following two reactions: (1) 2Hg(l) + O2(g)2HGO(s) AH° =…

A: the solution is as follows:

Q: Determine the enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s)…

A: To solve this we have to do some  mathematical operations with the given  two equations to get the…

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.