How many grams of water can be heated from 28.3°C to 41.8°C by the heat released from 83.5 g of lead that cools from 77.6°C to 28.9°C? g H2O(1) eTextbook and Media Hint Save for Later Attempts: 5 of 15 used Submit Answ

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A: Evaporation: The process in which liquid convert into vapor or gaseous form is called evaporation.…

Q: A chemist must add 3,352 kJ of heat to 2 mol solid Al2O3 to cause it to break down to form 4 mol…

A: Given: Heat supplied to solid Al2O3 = 3352kJno of moles of Al2O3 taken  = 2molno of mol of Al formed…

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Q: reaction for C,H, is 3) 12 CO, (g) + 6 H,O(1) + 6542 kJ and the heat produced from the burning is…

A: Final Temperature of water = 29.80°C

Q: How many grams of water can be heated from 28.3°C to 41.8°C by the heat released from 83.5 g of lead…

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Q: 3. What mass of water would need to evaporate from your skin in order to dissipate 1.7X10³ J of heat…

A: Given :  ∆Hvap = 2261 J/g  Heat given (q) = 1.7 x 105 J

Q: Help with q=mcchange in temp ?

A: We are authorized to answer one question at a time, since you have not mentioned which question you…

Q: How much heat will be absorbed by a 96.7 g piece of aluminum (specific heat = 0.930 J/g·°C) as it…

A: To solve this problem we will use the formula  Q = mC∆T  Where ,  Q = heat absorbed  m = mass of…

Q: How much energy is needed to completely boil away 147 grams of mercury if it starts at -50 °C?

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Q: Which of the following statements is incorrect concerning the thermochemical equation below? 2…

A: Exothermic reaction: The reactions in which heat energy is released is called an exothermic…

Q: Nitroglycerin, C;H5 (NO3)3 (1), is an explosive most often used in mine or quarry blasting. It is a…

A: A chemical reaction is a process in which one or more substances also known as reactants are…

Q: The specific heat capacity of solid iodine is 0.427 J/g °C. Calculate the final temperature (°C)…

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Q: What amount of heat (in kJ) is required to convert 10.1 g of an unknown liquid (MM = 67.44 g/mol) at…

A: we have to calculate the amount of heat needed to convert 10.1 g of the liquid to gas from 43.5oC to…

Q: at 1 atm how much energy is required to heat 55 g H2O(s) at −16℃ to H2O (g) at 161 C

A: Given,mass of solid water = 55.0 ginitial temperature  -16.0 oCFinal temperature = 161.0 oCFrom the…

Q: 10. How many grams of water (c=4.18 J/g-C) can be taken from 4°C t8 97 2133 JUUle 11. A 33.54 gram…

A: The heat of a reaction is the amount of energy released or absorbed during the course of a reaction.…

Q: The following information is given for mercury, Hg, at 1atm: AHvap(357 °C) = 59.3 kJ/mol boiling…

A: Mass of gaseous mercury = 46.6 g Boiling point of mercury = 357oC ∆Hvap = 59.3 kJ/mol Specific heat…

Q: Which of the following statements is incorrect concerning the thermochemical equation below? 2 AB…

A: We have been given a thermochemical  equation and change in enthalpy of this equation is also given.…

Q: 9. A piece of tin (specific heat 0.222 J/g*C) with an initial temperature of 80.0°C is placed in…

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Q: Prelaboratory Assignment: Investigation of Hess's Law Through Calorimetry 1. a) Calculate the amount…

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Q: Find the values for the enthalpy of formation (AHof) for CaCO3(s), CaO(s), and CO2(g).

A: The compounds given are CaCO3 (s), CO2 (g) and CaO (s).

Q: Ice cubes are made by taking heat away from water. Suppose you put 400.0g of 20.0 °C water in an ice…

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Q: When equal masses of each of the metals in the answers below absorb equal amounts of heat, which…

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Q: In the laboratory a student finds that it takes 19.7 Joules to increase the temperature of 10.3…

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Q: Write the chemical reaction used to determine the heats of formation for the following substance:…

A: The amount of heat absorbed or released when 1 mole of compound is formed from its respective…

Q: Consider the hypothetical thermochemical equation 3 A+ B 2 C for which AH = 59.3 kJ/mol. %3D If the…

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Q: A propane BBQ combusts propane as shown below: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (0 A,H =…

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Q: If the  ∆Hcomb of C4H10 = -2871 kJ/mol.  What would be the final temperature of 850.0 mL of water at…

A: Given : ∆Hcomb of C4H10 = -2871 KJ/mol. Volume of water = 850.0 mL Initial temperature of water =…

Q: The heat of formation of liquid methoxyethane (CH₂OC₂H₂) is -216.4 kJ/mol. Which of the following is…

A: Heat of formation is defined as the heat released when 1 mole of a compound is formed from its…

Q: How much heat (in kJ) will be absorbed by a 50.3 g piece of aluminum (specific heat = 0.930 J/g•°C)…

A: We know that   heat energy is given by     q = m* C* ΔT Given that   Mass of Al = 50.3 g   specific…

Q: A piece of metal weighing 98.4 g with a specific heat of 0.46 Jg-¹ °C-1 at 1028.6 °C is dunked into…

A: Given that,  The weight of the metal piece is mM = 98.4 g, The specific heat of the metal is CM =…

Q: Question #2 Calculate the amount of heat produced when 2.318 L of liquid acetonitrile (C₂H3N) is…

A: 4C2H3N(l) + 11O2(g)  ----->  8CO2(g) + 6H2O(g) + 2N2(g)    ∆H = -4989 kJDensity of liquid…

Q: A 200 g sample of copper (c = 0.385 J/g°C) and a 200 g sample of iron (c = 0.449 J/g°C) are both…

A: qCu  = mCu × cCu × ΔT = 200 g × 0.385 J/g.°C × (T2 – T1 ) = 200 g × 0.385 J/g.°C × (66.7 – 30.2 ) °C…

Q: 3. Using the Clausius-Clapeyron equation determine the vapor pressure of water at 50.0°C. The molar…

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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.