Which one of the equations below is an endothermic reaction? A) SrO (s) + CO₂ (g) → SrCO₃ (s)∆H° = -234 kJ/mol B) H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C) H₂ (g) + C (s) + N₂ (g) → 2 HCN (g) ∆H° = 270.3 kJ/mol D) 2 K (s) + 2 H₂O (l) → 2 KOH (aq) + H₂ (g) ∆H° = -393.1 kJ/mol

Q: Which one of the following reactions would produce the largest amount of heat per mole of hydrogen?…

A: Identify the reaction which would produce the largest amount of heat per mole of hydrogen.

Q: How much heat (in kJ) will be released (∆H) if 1.20 mol of SrO is mixed with 0.475 mol of CO₂ in the…

A:

Q: Using the equations 2 Sr(s) + O₂ (g) → 2 SrO (s) ∆H° = -1184 kJ/mol CO₂ (g) → C (s) + O₂ (g) ∆H° =…

A: If we multiply by any number or divide to the chemical reaction then ∆H will also multiply or divide…

Q: How much heat will be released (∆H) if 1.20 mol of SrO is mixed with 0.951 mol of CO₂ in the…

A: Let x be the number of moles at CO2 required by 1.2 mol of SrO 1.2 mol of SrO requires 1.2 moles of…

Q: Using the equations 2 Sr(s) + O₂ (g) → 2 SrO (s) ∆H° = -1184 kJ/mol CO₂ (g) → C (s) + O₂ (g) ∆H° =…

A: Given:

Q: How much heat (in kJ) will be released (∆H) if 1.20 mol of SrO is mixed with 0.717 mol of CO₂ in the…

A: Answer :-  ∆H° = -168 (kJ) When1.20 mol of SrO is mixed with 0.717 mol of CO2 , amount of heat is…

Q: Which one of the equations below is an exothermic reaction? A) CO₂ (g) → C (s) + O₂ (g) ∆H° = 394…

A: The energy is either absorbed or released during the chemical reaction. The negative sign of energy…

Q: Using the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C (s) + 2 F₂ (g) → CF₄ (g) ∆H° =…

A:

Q: Given the following thermochemical equations: 2NO(g) + O2(g) → 2NO2(g) ∆H° = -113.2 kJ 2N2O(g) +…

A:

Q: Consider this reaction: 2CH3OH(l) +  3O2(g)  →  4H2O(l) + 2CO2(g)   ∆H = –1452.8 kJ/mol Is this…

A: Given, thermochemical equation is: 2CH3OH(l) +  3O2(g)  →  4H2O(l) + 2CO2(g)   ∆H = –1452.8 kJ/mol…

Q: Using the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C (s) + 2 F₂ (g) → CF₄ (g) ∆H° =…

A: Some Basic rule. 1) On reverse of the reaction ,sign of ∆H value changes . 2) If any number is…

Q: How much heat (in kJ) will be released (∆H) if 1.20 mol of SrO is mixed with 0.555 mol of CO₂ in the…

A: Mol rationin SrO and CO2 is 1:1 . Excess SrO will remains in the solution.

Q: Given the data below, the energy released during the formation of ∆fHo  for the gas diborane, B2H6…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Using the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C (s) + 2 F₂ (g) → CF₄ (g) ∆H° =…

A:

Q: How much heat (in kJ) will be released (∆H) if 1.20 mol of SrO is mixed with 0.505 mol of CO₂ in the…

A: According to the balanced chemical equation, 1 mole of CrO reacts with 1 mole of CO2 . Also, 234 kJ…

Q: How much heat (in kJ) will be released (∆H) if 1.20 mol of SrO is mixed with 0.779 mol of CO₂

A:

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

A: Basic Rule  If any number is multiplied in reaction then that number is also multiplied in value of…

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.