A sheet of gold weighing 9.8 g and at a temperature of 17.8°C is placed flat on a sheet of iron weighing 20.3 g and at a temperature of 59.4°C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. °C

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A: The considered reaction is,

Q: Two substances, A and B, initially at different temperatures, come into contact and reach thermal…

A: The weight of substance A is 6.34 g.The initial temperature of substance A is 20.2˚C. The weight of…

Q: A sheet of gold weighing 10.0 g and at a temperature of 18.0°C is placed flat on a sheet of iron…

A:

Q: A sample of gas in a cylinder with a free-floating piston for a lid is heated. The gas gains 107 J…

A: given heat (q) = 107 J work done (w) = 23 J

Q: A 35.0-g sample of water at 25°C is mixed with 45.0 g of water at 88°C. Calculate the final…

A:

Q: solid, or to measure the energy of a solution phase reaction. A student heats 65.30 grams of gold to…

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Q: An engineering student wants to study the heat transfer between a 50 g of heated block of iron (cFe…

A:

Q: A sheet of gold weighing 9.3 g and at a temperature of 17.6°C is placed flat on a sheet of iron…

A: Given: mgold =9.3 g CAu = 0.129 J/g 0C Ti = 17.6 0C miron =21 g CFe = 0.444 J/g 0C Tiron = 55.3 0C…

Q: 4. A 5.00 gram sample of an unknown metal was placed in a beaker of boiling water (99.58 °C). After…

A:

Q: Consider the following data: When metals A and B are placed in contact with each other, which of the…

A: Answer is Option (B)

Q: If a 125 g sample of iron is heated to 250.0oC and then placed in 500.0 g of water at 25.0 oC in an…

A:

Q: A gas that works on the surroundings is equal to 432 J. At the same time, it absorbs 87 J of heat…

A: Work done by the gas on the surrounding means, the energy is reduced from the gas. Heat absorbed by…

Q: The table lists the specific heat capacities of select substances. Substance Specific heat…

A: The specific heat capacity is calculated using formula,

Q: When an alloy containing 20 g aluminum (c = 0.900 J g⁻¹ K) and 29 g copper (c = 0.385 J g⁻¹ K⁻¹) at…

A: Given that;   Mass of aluminum MAl  = 20g Heat capacity cAl  = 0.900 J/g°C  (unit correction)  Mass…

Q: A sheet of gold weighing 10.3 g and at a temperature of 10.0°C is placed flat on a sheet of iron…

A: The amount of heat absorbed (or released) by fixed amount of a substance to change its temperature…

Q: A metal object with mass of 29.0 g is heated to 97.0 °C and then transferred to an insulated…

A: Since the heat lost by metal + heat gain by water should be = 0 as no heat is lost in surroundings…

Q: 43.5-g sample of copper at 99.7 °C is dropped into a beaker containing 155 g of water at 18.6 °C.…

A: Given: mass of copper=  m1  = 43.5g temperature of copper = t1  = 99.7 deg C mass of water = m2 =…

Q: Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen…

A: Enthalpy is a state function  do it does not depend on the path it travelled as well as extensive…

Q: A 35.0-g sample of water at 25°C is mixed with 45.0 g of water at 88°C. Calculate the final…

A: Calculate for the final temperature of the mixture see step-2 for further Calculation and concept…

Q: A metal object with the mass of 24.1 g is heated to 97.0 *C and then transferred to an insulated…

A: Given: Specific heat of water = 4.18 J/g. oC Mass of metal = 24.1 g Mass of water = 86.9 g. Initial…

Q: A sheet of gold weighing 10.6 g and at a temperature of 15.3°C is placed flat on a sheet of iron…

A: Mass of gold weight = 10.6 g Temperature of Gold = 15.3°C Mass of iron weight = 21.2 g  Temperature…

Q: A 65.78 g piece of iron heated at 100.43 °C is placed in a coffee cup calorimeter contains 151.82 g…

A: heat lost by iron = ?

Q: We submerge a 25.0 g block of an unknown metal, initially at 97.8 °C, into 25.0 g of water initially…

A:

Q: A piece of unknown metal with a mass of 18.01 g is heated in boiling water to 98.9°C and then…

A:

Q: A sheet of gold weighing 9.3 g and at a temperature of 15.2°C is placed flat on a sheet of iron…

A: Since both the metals are in contact  hence the heat will transfer from the hot sheet to cold sheet…

Q: When 34.0 g of water at 24.0 °C are mixed with 46.0 g of water at 67.0 °C, what is the final…

A: Suppose the temperature of the final solution is X. When two such solutions are mixed where one…

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A: According to law of calorimetry heat absorbed  = heat released.  Copper has higher temperature so it…

Q: A piece of solid substance weighs 2.0g, and requires 100J to increase its temperature from 25.0…

A: Given: Mass of substance= 2.0 g T1= 25 C T2= 30.0 C Heat, q= 100 J

Q: A 20.8 g piece of metal has a specific heat of 0.52 J/g°C. It was heated to 99.5°C then placed…

A:

Q: Consider the thermochemical equation for the combustion of acetone (C3H6O), the main ingredient in…

A: Acetone reacts with oxygen to form carbon dioxide and water. The combustion reaction of acetone is…

Q: 79.8 grams of a metal that is at temperature 92.39 oC is placed in 186.3 mL of water at 19.79 oC.…

A: Here use thermal equilibrium concept. Here final temperature is 24.68 degree celcius, So metal…

Q: A metal object with mass of 20.5 g is heated to and then transferred to an insulated container…

A: when we mix to object then it grow from high temperature too low temperature . so apply principle of…

Q: A sample of silver metal is heated to 100.1 °C in a hot water bath until thermal equilibrium is…

A: Given that: mass of water = 52.483 g initial temperature of metal  = 100.1 °C final temperature of…

Q: 1. If 10 g of water at 52oC and 25 g of water at 10oC were mixed in an insulated container, what…

A: Please note- As per our company guidelines we are supposed to answer only one question. Kindly…

Q: A 991 g copper pan is removed from the stove at a temperature of 150 °C. It is then stacked on top…

A: Given: Mass of copper pan = 991 g Mass of aluminium sheet = 799 g Specific heat of copper = 0.387…

Q: The specific heat capacities for several substances are shown in the table. Substance Specific Heat…

A: Given :-  Substance          specific heat (J/g°C)  Iron                        0.45 Air…

Q: A 43.0-g sample of copper at 99.1 °C is dropped into a beaker containing 151 g of water at 18.7 °C.…

A: When copper is placed in water, the heat liberated from copper will be equal to the heat gained by…

Q: In a beaker 150.0 g iron is heated to the temperature of boiling water. In another beaker, 50.0 g…

A: The value possessed by all solids as well as liquids that gives heat needed to elevate temperature…

Q: Suppose that 26 g of each of the following substances is initially at 29.0 °C. What is the final…

A: Given: mass of substance = 26 g Initial temperature = 29°C Heat absorbed = 2.35 kJ  Standard data:…

Q: A piece of iron (mass = 25.0 g) at 368 K is placed in a styrofoam coffee cup containing 25.0 ml of…

A:

Q: Thirty grams of silicon at 80.0°C is added to 70.0mL of water at 20.0°C. Calculate the final…

A: Given: The mass of silicon = 30 g The initial temperature of silicon = 80.0 °C The volume of water =…

Q: A 250.0 g metal bar requires 5.866 kJ to change its temperature from 22 o C to 100.0 o C. What is…

A: The heat required (Q) to raise the temperature of any substance of mass m can be expressed as…

Q: A 837837 g copper pan is removed from the stove at a temperature of 150 °C. It is then stacked on…

A: Answer Final temperature         = 193.52 K (or) -79.63 °C Formula…

Q: For the following processes, calculate the change in internal energy of the system and determine…

A:

Q: An unknown hot metal at 122.41°C with a mass of 53.37g was mixed with 28.15g of water at an initial…

A: We have to calculate the  specific heat of the unknown metal.

Q: A fuel was used to heat water in a calorimetry experiment. When butane was burnt, 96070.0 J of heat…

A: Ans is given below

Q: A sheet of gold weighing 10 g and at a temperature of 18.0°C is placed flat on a sheet of iron…

A:

Q: A sheet of gold weighing 10.6 g and at a temperature of 15.3°C is placed flat on a sheet of iron…

A:

Q: 12.0 °C. 5. A sheet of gold weighing 10.0 g and at a temperature of 18.0 °C is placed flat on a…

A: Q = mCp∆T Where, Q = heat gained or lost m= mass of substance Cp = Specific heat capacity ∆T= Final…

Q: A 42.0 g sample of water at 100.00°C was placed in an insulated cup. Then 15.4 g of zinc metal at…

A: Given, A 42.0 g sample of water at 100.00°C was placed in an insulated cup. Then 15.4 g of zinc…

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.