A container with 78.2 grams of water at 32.0 C is placed into a deep freezer.  How may joules must be lost for the water to reach 1.00 C?  Round to the nearest whole number.  SpHt of water = 4.184 J/goC

Q: A 25.0 g block of copper (specific heat capacity 0.380 J/g-°C) at 88.0 °C is placed into 500.0 g of…

A:

Q: A 36.45 g sample of a substance is initially at 28.4 °C. After absorbing 1041 J of heat, the…

A: The mass of the substance is = 36.45 g The increase in the temperature of the substance is =…

Q: A sample of lead is heated to 189.4oC.  It is then placed in a cup containing 32.8 g water at…

A: The relationship between heat , specific heat capacity and change in temperature is given by the…

Q: 125g of hot Bismuth is placed in 45.0 mL of water (d = 1 g/mL)  at 23.0°C. What was the original…

A: Uisng the concept of conservation of energyHeat lost by hot Bismuth = Heat gain by water…

Q: For the chemical reaction H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol. What is the enthalpy (in…

A: The reaction given is, => H₂ (g) + F₂ (g) → 2 HF (g)…

Q: רPi How much heat will be released (AH) if 0.2037 mol of NH3 are mixed with 0.20 mol of O2 in the…

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Q: A 7.50-g sample of aluminum pellets (specific heat capacity = 0.89 J/°C-g) and a 12.00-g sample of…

A: The objective of the question is to determine the final temperature.It is given that,The mass of…

Q: If 40.0 g of hot water at 80.0oC is added to 60.0 g of cold water at 20.0oC, what is the final…

A: The final temperature is 44 oC

Q: A 12.3-g sample of granite initially at 76.0 ∘C is immersed into 21.0 g of water initially at 21.0…

A: Heat gained or absorbed by a substance = mass of the substance x specific heat capacity of substance…

Q: The combustion of 2.067 g of propanol (C, H,OH) increases the temperature of a bomb calorimeter from…

A: Given : Mass of C3H7OH combusted = 2.067 g Initial temperature of calorimeter = 298.00 K Final…

Q: A hot 111.6 g lump of an unknown substance initially at Substance Specific heat (J/(g.°C)) 150.0 °C…

A: By help of Following formula we can calculate the specific heat of the unknown Substance -   M1 C1…

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

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Q: A 140.0-g sample of water at 25.0°C is mixed with 101.1 g of a certain metal at 100.0°C. After…

A: Specific heat capacity of an element or a compound is equal to the amount of heat released or…

Q: A 1.00 g sample of MgCl2 produced a 10.00 °C increased in a calorimeter charged with 40.0mL of…

A: Mass of MgCl2 = 1.00 g Increase in temperature, ΔT = 10.00 °C Specific heat of MgCl2, C = 0.750…

Q: A 140.0-g sample of water at 25.0°C is mixed with 129.8 g of a certain metal at 100.0°C. After…

A: The hot metal will release the heat and that is taken by water and gets the equilibrium temperature.

Q: A gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and the rest propane…

A:

Q: A 27.95 g27.95 g sample of a substance is initially at 27.7 °C.27.7 °C. After absorbing 1867 J1867 J…

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Q: If 50.0 g H2O at 13.6 °C is combined with 244 g H2O at 93.7 °C, what is the final temperature of the…

A:

Q: A hot lump of 42.4g of copper at an initial temperature of 64.7 °C is placed in 50.0 mL H2O…

A: The given data to you is - mass of Cu = 42.4 g Volume of water = 50 mL Temp of Cu = 64.7 °C  Temp of…

Q: 2

A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…

Q: The specific heat capacity of silver is 0.24 J/°C·g. Calculate the energy required to raise the…

A: 1) Since the energy of heating process is given by  Q = m C  ΔT  where m = mass = 154 g C = specific…

Q: A 5.50-g sample of aluminum pellets (specific heat capacity = 0.89 J/°C·g) and a 18.00-g sample of…

A:

Q: A 150 g piece of iron was heated to a temperature of 47°C and then placed in contact with a 275 g…

A: Given,mass of iron=150 gmass of copper=275 gCp for copper= 25.46 J/(mol.°C)Cp for iron=25.09…

Q: 6. The heat of combustion of liquid ethylene glycol, C2H6O2 is -1189.2 kJ/mol. In an experiment 4.34…

A: All the details are explained in handwritten solution.

Q: A hot lump of 37.137.1 g of iron at an initial temperature of 95.6 °C95.6 °C is placed in 50.0 mL…

A:

Q: A glass contains 250.0 g of warm water at 78.0°C. A 50.0 g piece of gold at 2.30°C is placed in the…

A:

Q: A glass containing 200. g of H2O at 20C was placed in a refrigerator. The water loses 11.7 kJ as it…

A: Consider the given information is as follows; Mass of water = 200. g Heat loses (q) = -11.7…

Q: A piece of iron (mass 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of…

A:

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.