QUESTION 17 17. Calculate the amount of heat required to raise the temperature of 165g water from 12.0°C to 88.0°C. (Sp. Heat of water = 4.18 J/g°C) OA. 52.4 kJ O B. 1.93J OC. 60.7 kJ

Q: Mercury has the following physical properties: normal melting point = -39°C, normal boiling point =…

A: Normal melting point = -390CNormal boiling point = 3570CHeat of fusion = 2.33 kJ/molHeat of…

Q: Which of the following processes will require the largest amount of heat? a. Raising the temperature…

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Q: 0 g each of three metals, A, B and C absord the same amount of heat. The temperature of A increases…

A: Heat capacity is an intrinsic physical property of a substance . It is the measure of the amount of…

Q: What mass of oxygen is consumed when 285.5 kJ of energy is evolved from the combustion of a mixture…

A: Consider the given balanced reaction as;                          H2 g + 12 O2 g → H2O l…

Q: A 2.50 g block of iron is heated to 355.5 °C then plunged into 50.0 g of water at 25.0 °C. What will…

A: qw = -qm mw × cw × (Tf - Ti) = - { mm × cm ×( Tf-Ti) } 50 × 4.184 × (Tf - 25 ) = - { 2.50 × 0.444 ×…

Q: A 22.4 g piece of metal (C = 0.326 J/g oC) initially at 12 oC is placed in 35.9 g of water initially…

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Q: The conversion of graphite to diamond involves an internal energy change (ΔU) of 5.1 kJ mol-1 and a…

A: Given that, for the conversion of graphite to diamond involves an internal energy change (ΔU) of 5.1…

Q: Calculate AH for the reaction: Sg + Ozig) SO20 Se +02 (G 2 SO2 (9) + Ozig) 2 SO, 1g) A. 296.1 kJ AH=…

A: The value of ∆H depends on Stoichiometry of the thermochemical equation  If a chemical equation is…

Q: 3.) Calculate the change in temperature (AT). Use the SH heat table. a. 20.0 g of iron (Fe) that…

A: Formula , Q = m c Δ T  where, Q = heat transfer, m = mass of the substance, ΔT = change in…

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

A: The mass of the solution is the same as the mass of water and the mass of the 25.4 mL of water is…

Q: If Delta H = +32 KJ for a certain process, that process: a. is exothermic b can not occur c…

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Q: Calcuate the amount of heat in kJ neccessary to raise the temperatue of 50.0 g of a substance by…

A:

Q: 14. A 10.0-g sample of water requires 418 J of energy to increase in temperature by 10°C, whereas a…

A: Given: Qwater = 418 J Qcopper = 38.5 J Mass of water = mass of copper = 10 g ∆T = 100C

Q: The value of AH° for the reaction below is -126 kJ. The amount of heat that is released by the…

A: Given reaction is : 2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g) Standard change in enthalpy of the…

Q: A 23.2 g piece of metal (C = 0.455 J/g oC) initially at 14.2 oC is placed in 35.2 g of water…

A:

Q: When 1.00 g of AgCl is formed by the reaction in a coffee cup calorimeter, the temperature of 20.0 g…

A: Heat absorbed by water can be calculated by using the formula:Q = m.Cp.∆T where, Q = heat absorbed/…

Q: 16. What will be the final temperature of a 584−g sample of water, initially at 15.0 °C, after 53.4…

A: 584 g sample of water, initially at 15.0 °C. 53.4 KJ of heat have been added to it.Here we have to…

Q: A sample of 0.552 g of metal x (molar mass= 113 g/mol) was reacted with 150 mL of 1.0 M HCl in a…

A: Given - mass of metal x = 0.552 g             Molar mass of metal x = 113 g/mol            Volume of…

Q: Consider the following equations and data:  CH4(g)   +   2O2(g)    ------->     CO2(g)     +…

A: Given CH4(g) + 2O2(g) → CO2(g) + 2H2O (l) ΔH = - 890.4 kJ/mol  2H2O(l) → 2H2O(g) ΔH = +88.0 kJ/mol

Q: Calculate AG° for the electrochemical cell Fels) I Fe2*(aq) || Sn (aq) i Sn2(aq) | Pt(s). Multiple…

A: Gibbs free energy change can be used to determine the spontaneity of a chemical reaction. It can be…

Q: 8.A sample of 1 mol ideal gas is heated at constant pressure, when the temperature is raised 1 K,…

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Q: 2. Use the data on the left side of Table 1 to perform the calculations necessary to complete the…

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

Q: 76 of 76 I Review I Constants I Periodic Table Part A Assuming that all the energy given off in the…

A:

Q: 24. Consider the following thermochemical equation sometimes used for H2S production: S8(s) + 8…

A: The given reaction is :  S8(s) + 8H2(g) = 8H2S(g)  ∆Hrxn = -20.2 kJ  From the reaction it is clear…

Q: 7. Which of the following technologies are considered non-renewable energy sources? Choose ALL that…

A: The phenomenon of electrons occupying orbitals at the same energy sublevel singly before any orbital…

Q: Calculate the total enthalpy change (kJ) for the following reaction:   H2O (s, 90 g, –10. oC)…

A: In the above process, 3 steps are involved 1) Heating of 90 grams ice from –10 oC to 0 oC  2) fusion…

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.