Chapter 5 Review How much energy is needed to boil 45.0g of water at its boiling point? Water's heat of vaporization is 40.65KJ/mole. O 58.3kJ O 10,200 kJ O 1830kJ O 102kJ

Q: Using the reverse reaction, how much heat is required to produce 44.8g of NO using the following…

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Q: The heat of combustion for 1.00 mole of carbon to carbon dioxide is -410. kJ. How many kJ of heat…

A: Given : Moles of carbon = 1 mole

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: If 7.90 kJ of heat is needed to raise the temperature of a sample of metal from 15 °C to 20. °C, how…

A: The heat transfer is given by q = m x c x ΔT where: q = heat gained or lost (in Joules) m = mass of…

Q: Consider the Sublimation of dry ice (solid carbon dioxide). The value of deltaHsub for CO2 is…

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Q: According to the scheme below, How much energy is required to evaporate 54.06 g water (Molecular…

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Q: How many kilojoules (kJ) of energy would be required to raise the temperature of 200.0 grams of…

A: Given datas ;  m = 200.00 g  Ti = 25.00°C  Tf = 100.00°C  c = 4.184 J/g°C  q = ?

Q: How much heat, in kJ, will be absorbed by a 25.0 g piece of aluminum (specific heat = 0.930 J/g･°C)…

A: Hi there! Since you have posted multiple questions, we will answer the first question for you.

Q: How much heat, in kJ, will be absorbed by a 25.0 g piece of aluminum (specific heat = 0.930 J/g °C)…

A: Now we can use the formula:q=mcΔTexplanationwhere: q is the heat absorbed in (J)m is the mass of the…

Q: An arctic explorer is trying to create drinking water by converting an ice ball into liquid. The ice…

A: Given that : The mass of ice = 225 g The initial temperature of ice = -23°C The final temperature of…

Q: 8. A piece of unknown metal with a mass of 5.19g is heated to 100.00°C and dropped into 10.0mL of…

A: Heat released or absorbed (Q) = m . s . ∆T Where, m = mass of substance, s = specific heat of…

Q: 6. Use Hess's Law and the following data: Sro(s) à Sr (s) + 1/20₂(g) SrO(s)+ CO₂(g) à SrCO3(s) 2…

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Q: Consider that 53.0 g of water at 63.28°C was cooled by the removal of 900J of heat. Calculate the…

A: To calculate the final temperature of water , we would use formula : q = m × C × dT  where , q =…

Q: Which of these are TRUE for ENDOTHERMIC reactions? 1. The temperature of the surroundings is…

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

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

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Q: What is the definition of the specific heat capacity of a substance? the amount of heat required to…

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Q: 1. Calculate the energy (in kJ) required to heat 0.613 grams of water from -48.4 ℃ to -14.1 ℃. 2.…

A: Given,1. Mass of water = 0.613 g.Initial temperature= -48.4 ℃ Final temperature=-14.1 ℃.2.Mass of…

Q: 1. Normal body temperature is 98.6 °F. What is this temperature in °C? A person with a "fever" has a…

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

Q: How much energy is needed to raise the temperature of 325g of water by 10.0 degrees? The specific…

A: Given  Mass of water = 325 g = m  Specific Heat of water = 4.184 J/g°C ∆T = 10 °C

Q: Calculate the total energy in kJ required to change the temperature of 238 g water from 19.0  oC to…

A: Since the boiling point of water is 100 oC and melting point is 0 oC Hence during the temperature…

Q: A 1.67-g sample of solid silver reacted in excess chlorine gas to give a 2.21-g sample of pure solid…

A: The equation for the formation of AgCl(s) is: Ag(s) + 1/2 Cl2(g)  ----> AgCl(s) ; ∆Hof  = ??…

Q: 03 Multiple Choice Which of the following is a quantitative measure of disorder?

A: The entropy  is a measure of the amount of energy which is unavailable to do work. It also suggests…

Q: 11. A 45.0 g block of iron that has an initial temperature of 340 °C and a 45.0 g block of gold that…

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Q: Tow many kilojoules of energy will be needed to decompose 10.8 g of N205 gas? N205 (g) + 110 kJ-> 4…

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Q: If you have 0.113398Kg of iron. How much heat, in joules, must be added to raise their temperature…

A: Given,specific heat of iron is 0.452 J/g °CInitial temperature =16 °CFinal temperature = 125 °CMass…

Q: Juan freezes a bottle of water to ice (500.mL) in preparation for a road trip. How much heat can be…

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Q: Calculate the amount of energy (in kJ) required to heat 100. g of water from 20.0 ºC to 35.0 ºC?…

A: Thermodynamics is branch of chemistry which deals with heat gained or heat lost by the system.

Q: Copper metal has a specific heat of 0.385 J/g°C. Calculate the amount of heat required to raise the…

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Q: A flask containing 1200 g of water is heated, and the temperature of the water increases from 25°C…

A: Mass of water = 1200 g Temperature rises from initial temperature, Ti = 25°C To final temperature,…

Q: temperature of a 11.8 g sample of calcium carbonate [CaCO3 (s)] increases from 24.8 °C to 38.0 °C.…

A: Specific Heat capacity is amount of heat required to increase one gram of substance by one degree…

Q: What heats up the fastest when exposed to the same amount of energy?A.Sand (c = 0.830 J/g•oC)…

A: Specific heat (c) of a substance is defined as the amount of heat required by a substance to raise…

Q: A metal pellet with mass 25.0 g and temperature 90.0 °C is dropped into 100.0 g water originally at…

A: Given:  Mass of metal = 25.0 gm  Initial  temperature = 90.0 °C  Mass of water = 100 gm  Initial…

Q: Calcium carbonate decomposes at high temperatures to form carbon dioxide and calcium oxide,…

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Q: Study Guide Mix n Match:       1. Temperature is the measure of the Total energy of a substance.…

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Q: The amount of energy needed to heat 2.00 g of carbon from 50.0oC to 80.0oC is 42.56 J. The specific…

A: Given, mass of Carbon = 2.00 g  Heat energy = 42.56 J  Specific heat capacity  = ?

Q: A balloon is filled with two gases that undergo a reaction. The temperature inside the balloon…

A: We are given a situation in which two gases react in a balloon and asked  to predict whether the…

Q: When 50. g of solid carbon dioxide (dry ice) sublimes 28.6 kJ of heat are required. How much heat…

A: This problem is solved by means of the rules of unitary method.

Q: 4. The specific heat of water is quite high at 4.184 J/gC. Explain how life on this planet would be…

A: The amount of heat required to increase the temperature of the 1 g of the substance by 1 degree is…

Q: an 33.777g piece of metal is heated in a hot water bath at 98.5°C and then cransferred to a…

A: Given, mass of metal, m =33.777 g temperature of hot water bath T1 =98.5°C Volume of water in coffee…

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A: The specific heat capacity for a given chemical substance or a solution refers to the amount of 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.