How many grams of C₆H₆ liquid must decompose according to the following chemical equation to transfer 430kJ of heat?

Q: Suppose 4.00 x 103 m3 of natural gas is used in a year to heat a certain building. Assuming that…

A: Number of moles of methane can be calculated using ideal gas equation:

Q: How much heat is evolved when 30.g of magnesium is burned in excess oxygen gas given thereaction…

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Q: How many grams of C5H12

A: ∙Given:- mass =1.24kg or 1240g                    T1 Initial temperature=23.6°C…

Q: 10. What would be the final temperature if 55.0g of H2O at 30°C is added to 45.0g of H20 at…

A: The amount of energy going out of the warm water is equal to the amount of energy of the cool water.

Q: Using the enthalpy change of -1594 kJ, what is the amount of heat absorbed or released when 1.10 L…

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Q: When one mole of C6H6C6H6 is burned, 3.27 MJ3.27 MJ of heat is produced. When the heat from burning…

A: Given : burning 1 mole of C6H6 produces heat = 3.27 MJ = 3.27 X 106 J…

Q: What is the final temperature when a 5.0 g sample of brass initially at 25 oC absorbs 75 J of heat?…

A: Equation for finding the heat absorbed by brass is as follows. Q=mc∆TQ=heat absorbed by brassm=mass…

Q: (a) Convert 41.3 L atm to kcal. (Use dimensional analysis)  (b) Convert –279.67°F to K. (C)The…

A: Bond enthalpy: It can be defined by saying that the amount of energy required to break the bond for…

Q: What would be the final temperature if 50.0g of H2O at 30.0C was added to 40.0g of H2O at 90.0C?…

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Q: Zinc metal reacts with hydrochloric acid according to the following reaction: % Zn (s) + HCI (aq) →…

A: The reaction given is, Given: Mass of Zn reacting = 0.9807 g. Concentration of HCl = 0.250 M Volume…

Q: Measurements show that the energy of a mixture of gaseous reactants decreases by 153. kJ during a…

A: According to the first law of thermodynamics, the total heat change of a system at constant pressure…

Q: What quantity in moles of H₂ are required to give off 2501 kJ of heat in the following reaction? N₂…

A: The objective of the question is to find out the quantity in moles of H2 required to give off 2501…

Q: When 221 grams of water at a temperature of 25oC is mixed with an unknown mass of water at a…

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Q: Please determine the enthalpy (in kJ/mol) of the balanced thermochemical equation when 2.15 g of…

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Q: 2 NH4CIO4(s)→ N₂(g) + Cl₂(g) + 2 O2(g) + 4 H₂O(g) AH = -375.6 kJ The enthalpy of formation of H₂O(g)…

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Q: When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas…

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Q: type of chemical reaction

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Q: How much heat has to be added to 235 g of iron at 25.0° C to raise the temperature of the iron to…

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Q: Measurements show that the energy of a mixture of gaseous reactants decreases by 177. kJ during a…

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Q: Using the equations H, (g) + F, (g) → 2 HF (g) AH° = -79.2 kJ/mol C (s) + 2 F, (g) → CF, (g) AH° =…

A: Since you have posted multiple questions we will solve the first question for you. To get the…

Q: TRUE/FALSE: the following reaction is a formation reaction: 2C(s) + 4H2(g) → 2CH4(g)

A: Formation reaction: A formation reaction is the formation of one mole of a substance from its…

Q: Determine the final temperature of a 377 g sample of iron when 2.64 kJ of heat is added. The initial…

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Q: What quantity of heat (in kJ) will be released if 0.5649 mol of NH, are mixed with 0.200 mol of O,…

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Q: The specific heat of mercury is 0.140 J/g°C. Calculate the heat necessary to raise the temperature…

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Q: a) A person drinks four glasses of cold water (3.0°C) every day. The volume of each glass…

A: Given: volume=2.6×102 mLInitial temperature=3.0oCFinal temperature=37oC To find: Heat supplied

Q: When one mole of C6H6C6⁢H6 is burned, 3.27 MJ3.27 MJ of heat is produced. When the heat from burning…

A: From the given in the question, The number of moles of C6H6 is given by = 1 mole The heat released…

Q: A 402 g sample of silicon is subjected to a temperature change of -800.29 K while releasing 228980…

A: Heat released by the material = mass × specific heat capacity ×temperature change Where, heat…

Q: access the section in your eText. Part A Titanium reacts with iodine to form titanium(III) iodide,…

A:

Q: A 5.90-g chunk of potassium is dropped into 1.00 kg water at 24.7°C. What is the final temperature…

A: 1.A 5.90-g chunk of potassium is dropped into 1.00 kg water at 24.7°C. 2. Tobfind out the final…

Q: If 40.0 kJ of energy is absorbed by 500.0 g of water at 10.0 oC, then what is final temperature of…

A: Q = m . s . (T2-T1)

Q: A 27 g aluminum foil pan is used to roast vegetables.  The pan is put into a cold oven at 22 oC .…

A: The heat released or absorbed (q) by a substance when the temperature of that substance is raised is…

Q: What is the heat capacity of 2.00 moles of liquid water?

A: Given: heat capacity of 2.00 moles of liquid water   To find: find capacity of 2.00 moles of liquid…

Q: Determine the total heat absorbed by the reaction, in kJ, if 2.50 g of O, is required to fully…

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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.