2) The Columbic potential (kj/mol) of the ionic bond between Na*1 and Cl-1 ions is 595kj/mol. Calculate the distance between two ions. Use ɛ0 = 8.854 x 10-12 C²J-lm-! e = 1.602 x 10-19 C Ipm = 10-12 m

Q: 5) C-O and O-H bonds are stronger than C-C and C-H bonds, because C-O bonds and O-H bonds S1eolar.…

A: Answer: Chemical reaction is a process in which old bonds get broken and formation of new bonds take…

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: NaCl has a lattice energy of -787 kJ/mol. Consider a hypothetical salt XY. X3 + has the same radius…

A: The lattice energy of NaCl is -787 kJ/mol. The formula required to calculate lattice energy is as…

Q: 12. Estimate the enthalpy change for the reaction 2CO + O2 →2CO2 given the following bond energies.…

A: The chemical reaction :  2CO + O2  -----> 2CO2   The binding energy of :   C≡O = 1074 KJ/mol. O=O…

Q: The equation for the reaction of nitrogen and hydrogen to form ammonia is shown below. N,(g) + 3H,…

A: Given N2 +3H2 →2NH3 △H = - 97 KJ/mole The enthalpy of H-H and N≡N are 436 and 941

Q: Using the table of standard formation enthalpies that you'll find under the ALEKS Data tab,…

A: The standard reaction enthalpy of a reaction is given by   ∆Hrxn°=∑∆H° of the products -∑∆H° of the…

Q: The equation for the reaction of nitrogen and hydrogen to form ammonia is shown below. N,(g) +…

A: Reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g)   ∆H° = (sum of bond enthalpies of reactants - sum of bond…

Q: KCl has a lattice energy of −701 kJ/mol. Consider a generic salt, AB, where A2+ has the same radius…

A: The Lattice energy of KCl is given as −701 kJ/mol. It is composed of  K +  and Cl- ions. The given…

Q: For items 1-3, refer to the equation: CH4(9) + 202(9) → 2H2O1) + CO2(9), with AH equal to -809.94…

A: 1) , 2) , 3)  Given :-  The given reaction is CH4(g) + 2O2(g) → 2H2O(l) + CO2(g) ΔH = -809.94 kJ/mol…

Q: 8. Determine the enthalpy for the following reaction, given AH (NH3(g)) =-46.1 kJ/mol, AH, (NO(g)) =…

A:

Q: 8 An energy cycle is drawn for the following reaction. Br₂(1) + 3F₂(g) → 2BrF3(1) +698kJ 2Br(g) +…

A: The objective of the question is to calculate the average bond energy of the bond in .

Q: 1/2 N₂(g) + 1/2 O₂(g) → NO(g) kJ/mol-rxn Enthalpy change =

A:

Q: iven the data below, calculate the enthalpy of reaction (in units of kJ) for the reaction:  2 C2H2…

A: Enthalpy of a reaction = Sum of enthalpies of products – Sum of enthalpies of reactants

Q: Bond Average Bond Enthalpy (kJ/mol) N-H 391 H-H 436 N= N ? (b) Based on the average bond enthalpies…

A: Answer: In this question with the help of standard enthalpy of formation of ammonia and given bond…

Q: How much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar?…

A: The objective of the question is to find out how much the sodium-in-water demonstration raised the…

Q: For the reaction: C₂H₂(g) + 50₂(g) → 3CO₂(g) + 4H₂O(g) Part 1 of 2 Predict the enthalpy of reaction…

A:

Q: Use bond enthalpies in the table below to estimate AH for each of the following reactions. Part B…

A:

Q: Using the information provided, determine the enthalpy (in kJ/mol) for the reaction 2 NH₃ (g) + 3…

A: The enthalpy of a reaction is the enthalpy change between products of the reaction and the reactants…

Q: Calculate the standard enthalpy change for the following reaction: CH4(g) + 2 O₂(g) → CO₂(g) + 2…

A:

Q: 3. Write out the chemical equation for the enthalpy of formation of NaCl(s).

A: NaCl is formed by reaction of Na(s) ans Cl2(g). With the help of this reaction we can calculate…

Q: * Bond energy in CO2 is equal to 799 kJ/mol. ▾ Part B Bond Bond energy (kJ/mol) Bond Bond energy…

A:

Q: The following reaction is endothermic. KCIO4(s) K(s) + 1/2 Cl₂(g) + 2 0₂(g) AH(1) = 433 kJ Calculate…

A: Recall the given reaction,                         KClO4 s  →  K s  +  1/2 Cl2 g  +  2 O2 gThis is…

Q: 12. Consider the following process. + 2H,O(e) AH = -802 kJ %3D CH4 (8) + 202 (8) 2 CO2 (8) A) Is the…

A: We have to predict the change in enthalpy and it's nature.

Q: A compound such as calcium carbonate can decompose by absorbing energy. This reaction can be written…

A:

Q: Use the molar bond enthalpy data in the table to estimate the value of AHin for the equation rxn…

A:

Q: Methane is the main component of natural gas. Using the given reaction enthalpy, calculate the heat…

A:

Q: In a calorimetry experiment 5.6 g of potassium hydroxide is dissolved in 400 mL water in a thermos…

A: In the given question we have to calculate the enthalpy change of the following,  first of all, we…

Q: Table 4. Enthalpy of solution of salts data and calculations Table 4. Enthalpy of solution of salts…

A:

Q: For the chemical reaction Ca (s) + 02 (g)→CAO (s) AH° = -635 kJ/mol. What is the enthalpy for the…

A: Given reaction,      Ca(s) + 1/2 O2(g) → CaO(s)       ∆H0 = - 635 kJ/mol

Q: Use the provided table of bond energies to calculate the enthalpy change (ΔHrxn) in kJ for the…

A:

Q: Determine the enthalpy for the following reaction, given A (NH3(g)) = -46.1 kJ/mol, AH (NO(g = +90.3…

A:

Q: The standard enthalpy change for the following reaction is -602 kJ at 298 K. Mg(s) + 1/2O₂(g) →…

A:

Q: CSCI has a lattice energy of -657 kJ/mol. Consider a generic salt, AB, where A²+ has the same radius…

A: Lattice energy is the energy required to dissociate the salt of type AB into the ions of A+ and B-.…

Q: When 3.8 g A are reacted with 8.5 g D,  according to the balanced chemical equation below, 33 kJ 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.