A 466 g of water is heated from 8.50C to 74.60C. Calculate the amount of heat absorbed (in kilojoules) by water. *

Q: The specific heat capacity of graphite is 0.71 J/°C g. Calculate the energy required to raise the…

A: The information given in the question is as follows: Specific heat capacity of graphite, c = 0.71…

Q: How much heat (in kJ) is required to raise the temperature of a 525.0 mL sample of water from 22.1 C…

A: The heat required to raise the temperature is directly proportional to the mass of sample and the…

Q: A 149.6-g sample of a metal at 75.0°C is added to 149.6 g H2O  at 14.0°C. The temperature of the…

A: Given For metal, mass(m)=149.6 g Initial temperature(Ti)=75℃ Final temperature(Tf)=30℃ Specific…

Q: How much heat is needed to raise the temperature of 100.0 grams of water from 25.0°C to 55.0°C?…

A: Information about the question

Q: When 12.29 g of finely divided brass at 95.0 °C is quickly stirred into 40.00 g of water at 22.0 °C,…

A: Given, Mass of brass= 12.29 g Temperature = 95.0°C Mass of water = 40.00 g the temperature of water…

Q: Calculate the energy supplied to 0.070 kg of water contained in a copper cup of mass 0.080 kg. The…

A: It is given that 0.070 kg of water is contained in a cup of copper which has a mass of 0.080 kg, and…

Q: How much heat is needed to raise the temperature of a 2.5 g piece of copper wire from 20. °C to 80.…

A: When the temperature rise of a 1 g of substance takes place by 1°C, some amount of heat is required…

Q: iberated (In KJ) from 3b6 g of mercury when It cools from to 12.0°C. The specific heat of mercury is…

A: Heat absorbed can be calculated by using the formula :                       q = ms∆Twhere, q is…

Q: he heat change that accompanies the formation of 1.00 mol of carbon dioxide from its elements is…

A: The standard enthalpy of formation or standard heat of formation of a compound is the change of…

Q: If 85.1 cal of heat are added to 10.0 g of water (specific heat = 4.184 J/g oC) at 30.0 oC, what is…

A: * Heat added = q = 85.1 cal (1 cal = 4.814 J ) q = 85.1 × 4.814 J = 409.67 J * Mass of water = m =…

Q: A 6.22 kg piece of copper metal is heated from 20.5 °C to 324.3 °C. Calculate the heat absorbed (in…

A: Given data,  mass of copper metal = 6.22kg= 6220g Specific heat of copper = 0.385 J/g°C Change in…

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

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.