How much heat, in calories, is required to heat a 18.4 g ice cube from -23.0 °C to -1.0 °C? Specific heat of ice is 2.108 J/g°C, 1 calorie =4.184 J 204 853 135

Q: How much heat (in kJ) will be absorbed by a 51.5 g piece of aluminum (specific heat = 0.930 J/g °C)…

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Q: How many kJ of heat is needed to raise the temperature of 0.250 L of water in t liquid phase from…

A: Volume of water V = 0.250 LT1 = 24.6 oCT2 = 46.2 oC

Q: How much heat must be added to a 8.21 g sample of gold to increase its temperature from 25 oC to…

A: We know that Q = m×C×∆T Q = heat m = mass C = Specific heat ∆T = change in temperature m = 8.21g C =…

Q: neat re

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Q: How much heat, in joules, must be added to a 75.0 g block of a metal alloy with a specific heat of…

A: Given, Mass of the substance, m = 75.0 g Initial temperature, T1 = 25 oC Final temperature, T2 = 775…

Q: A calorimeter contains 2.50 kg g of water at 37.0 °C. A 225-g sample of ice (at -20.0 °C) is added…

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Q: 10 g of solid NH4Cl is mixed with 50 g of water in a calorimeter that absorbs no heat. The…

A: The heat of solution, also known as the enthalpy of solution, is the heat energy absorbed or…

Q: 107 g of Cu at 108.9\deg C was added to 258.7 g of H2 O at 17.4\deg C. If the specific heat of…

A: The objective of the question is to calculate the final temperature of the water and copper mixture.

Q: When 6.72 grams of potassium chlorate (KCIO3) are dissolved in 120.0 grams of water at 25.0 °C in an…

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Q: How much heat, in calories, must be added to a 102.0g iron block with a specific heat of 0.449 J/g…

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Q: Calculate the final temperature that results when A 12.6 g sample of water at 22.9 0C absorbs 875 J…

A: The given two problem can be solved by this equationQ=m.c.△TWhereQ=Amount of heat absorbed or lost…

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: Which statement best defines specific heat? The amount of heat required to increase the temperature…

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Q: the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will…

A: Specific heat capacity is amount of heat needed to increase the temperature of one gram of substance…

Q: A block of rhenium metal (specific heat =0.0329 cal/ gC) is heated to 88.2C and then dropped into…

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Q: A solution is made by mixing 232.0 mL of ethanol initially at 12.7 ∘C with 232.0 mL of water…

A: According to Law of calorimetry,amount of heat released by the substance having higher temperature…

Q: A (4.1700x10^1) g sample of water (C = 4.18 J / g ºC) initially is at (5.110x10^1)ºC. What is the…

A: According to the equation, Q=mcdTQ=Heat absorbed or releasedc=specific heat capacitydT=Change in…

Q: The specific heat of aluminum is 0.897 J/g·°C and the specific heat of water is 4.18 J/g·°C.  If a…

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Q: When a 45.0 g sample of an alloy at 100.0°C is dropped into 100.0 g of water at 25.0°C, the final…

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Q: The specific heat capacity of liquid mercury is 0.14 J/g-K. How many kilojoules of heat are needed…

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Q: 1) A 0.416 g sample of KCl is added to 56.5 g of water in a calorimeter. If the temperature…

A: The heat capacity of the resulting solution is 4.18 J/goC, which states that 4.18 J of energy will…

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.