O An office worker claims that a cup of cold coffee on his table warmed up to 80°C by picking up energy from the surrounding air, which is at 25°C. Is there any truth to his claim? Does this process violate any thermodynamic laws?

Q: lution of HI was found to have a pOH of 13.35 at 25 °C. What is the concentration of HI? a. 0.52 M…

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Q: Determine ∆U in a chemical system that absorbs 50.5 kJ of heat from the surroundings and performs…

A: According to the first law of thermodynamics,

Q: A 100.0 g piece of metal at 100°C is placed in contact with 50.0 g of water (s = 4.184 J g–1 °C–1)…

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Q: Consider the reaction N2(g)+3H2(g)→2NH3(g),N2(g)+3H2(g)→2NH3(g), ΔHΔH =−92.3kJ mol−1=−92.3kJ mol−1…

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Q: Calculate ΔH⁰298  (in kJ) for the process P(s) + 5/2 Cl2(g) → PCl5(g) from the following information

A: Hess's law :  This law states that " the change of enthaply in a chemical reaction is the same ,…

Q: 150.0 mL of 0.500 M hydrochloric acid is mixed with 350.0 mL of 0.150 M barium hydroxide in a coffee…

A: Given : concentration of HCl = 0.500 M Concentration of Ba(OH)2 = 0.150 M Volume of HCl solution =…

Q: A sample of hydrogen gas is kept in a container with a piston. Recall that 1 L atm = 101.3 J. If the…

A: Given data :  Volume (V1) = 1.0 L  Volume ( V2) = 4.5 L  To calculate : work done Against a vacuum…

Q: Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is…

A: Heat given Q = 25.0 kJ  Initial volume Vi = 12.00 L  Final volume Vf = 6.00 L Constant pressure P =…

Q: In an experiment to determine ΔHfusion of ice, a student added 29.04 grams of ice originally at…

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Q: Use the data below and Hess’ law to calculate the ΔrHo for the overall reaction: C2H4(g) + 6F2(g) →…

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Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 664.0 mg sample…

A: To find the molar heat capacity, we need to use the formula which contains mol, specific heat and ∆T…

Q: 9.45 mol of a monoatomic perfect gas with an initial volume of 10.33 L and temperature of 204 K…

A: 1) Constant external pressure so, P1 = P2 = 1.35 atm Number of monoatomic gas, n = 9.45 mol Initial…

Q: Describe the relationship of enthalpy, work, and internal energy. Calculate the ∆U for these…

A: First law of thermodynamics state that energy can neither be created nor be destroyed but can be…

Q: Part A The value of AS° for the catalytic hydrogenation of acetylene to ethene, C2H2 (g) + H2 (g) →…

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Q: 5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the…

A: The question can be solved by giveb formula,  Q=m×C×dT where Q = heat energy (Joules, J),  m = mass…

Q: What is the work performed when a gas expands from 0.66 L to 2.33 L against an external pressure of…

A: We have been given initial volume, final volume and external pressure We have been asked the work…

Q: When 2.18 g of copper(II) chloride (CuCl2) is dissolved in 119 g of water in a styrofoam calorimeter…

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Q: Reaction 1: 20F2 (g) → O2(9) + 2 F2 (9) AH=-49.4 kJ Reaction 2: N2 (g) + 202(g) → 2NO2 (g) AH=+66.4…

A: When the gibbs free energy change is positive then the reaction is spontaneous and when the gibbs…

Q: Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 1.43 g of…

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Q: Thirty grams of ice at 0.0°C is added to a Styrofoam cup containing 150 mL of water at 65°C. After…

A: Heat released by water, q = ms∆T  q = 150 x 1 x ( 65 - 40 ) q = 3750 cal   Heat required to raise…

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 the change in internal energy (ΔU) for a system that is giving off 25.0 kJ of heat and is…

A: The first law of thermodynamics states that the change in internal energy of a system equals the net…

Q: suppose that a system gives off 50.1 kJ of heat and has 300. J of work done on it.   What is the…

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Q: Nitrogen oxide (NO) has been found to be a key component in many biological processes. It also can…

A: The given is reaction for formation of NO2 NO(g) + ½O2(g) → NO2(g) ΔH = –57.0 kJ We are to find out…

Q: Sam is having a great deal of difficulty with thermodynamics, particularly when systems are not…

A: When system is ideal and when cooked pizza is delivered to sam, it is not going to cool by external…

Q: In a system composed of nitrogen gas in a cylinder fitted with a piston, when 2.00 kJ of energy is…

A: Answer:- This question is answered by using the simple concept of calculation of change in internal…

Q: The molar heat capacity of silver is 25.35 J mol−1 ∘C−1. Find how much energy would it take to raise…

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Q: 20. Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and…

A: The problem is asking us to calculate the change in internal energy (ΔE) of a system. We are given…

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.