The temperature of a sample of water changes from 1000 to 20°C when the sample absorbs 418 joules of heat. What is the mass of the sample? DEMCAT

Q: A sample of water with a mass of 38.50 grams absorbs 2.950 kJ of heat energy. if the initial…

A:

Q: 12.755 g of a mental initially at 99.0 degrees C are placed into 75.0 g of water initially at 23…

A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…

Q: 500.0 g of water in its liquid phase loses 5,892 J of heat. If it started at a temperature of 25.0…

A: We have given that  The mass of water = 500g  Heat release in liquid phase = 5892J  Initial…

Q: A 18.32 g piece of metal absorbs 86.73 J of heat while rising from 28.01°C to 50.52°C. Calculate the…

A: Specific heat :-  The amount of heat required to rise the temperature of one gram of a substance…

Q: In the specific heat equation, what unit must temperature be? Celsius O Fahrenheit Kelvin Joules

A: First we have to know about Specific heat. Specific heat : It is heat required to raise the…

Q: What is the specific heat of an unknown liquid if heating a 15.0 g sample with 200.0 J of heat…

A:

Q: 1. If 200. grams of water is to be heated from 24.0°C to 100.0°C to make a cup of tea, how much heat…

A: Given that:                                             Mass of water = 200 g…

Q: If 75.0 grams of water is heated from 32.6°C to 78.9°C, how many kilojoules of heat does the water…

A: Given - - > Mass, m = 75 g Initial temperature, T1 = 32.6°C Final temperature, T2 = 78.9°C…

Q: How many joules are required to heat 180g of water from 20c to 35c. The specific heat of water is…

A:

Q: The specific heat of copper is 0.093cal/g °C, and the specific heat of silver is 0.057 cal/g °C.  If…

A: Specific heat is the amount of heat required to raise the temperature of a substance by 1°C/K.Its SI…

Q: Assuming no heat loss by the system, what will be the final temperature when 51.0 g of water at 10.0…

A: The final temperature has to be calculated. The mass of water at 10.0°C is 51.0 g. The mass of water…

Q: If 980 calories of energy as heat are transferred to 62.85 grams of a substance with an initial…

A: The amount ot heat is required to raise the temperature of body of unit mass to one degree Celsius…

Q: How much energy does it take to heat a cup of water (242 g) from room temperature (21.0°C) to its…

A: Step 1) Specific heat says that how much heat is required to raise that temperature 1 g of a sample…

Q: if 624J of heat is added to 30.2g of water at 24.3°c, what will the final temperature of the water…

A: The amount of heat added is = 624 J The initial temperature of the water is = 24.3oC The mass of…

Q: 81. An iron nail with a mass of 12 g absorbs 15 J of heat. If the nail was initially at 28 °C, what…

A: Given data mass of iron nail : m = 12 g heat absorbed : Q = 15 J Initial temperature : T1=28°C…

Q: How much heat in joules is needed to raise the temperature of 4.5 L of water from 0°C to 89.0°C?

A: Formula for heat taken to change the temperature is:

Q: Calculate the initial temperature of a 332.5g sample of water that released 32,000J of heat and had…

A: Given: The final temperature is 3.57 °C. The heat released is 32000 J. The mass of water is 332.5 g.…

Q: True or False? If 25 grams of hot water are added to 35 grams of cold water, the heat lost by the…

A: The given statement is TRUE here

Q: A sample of iron absorbs 77.8 J of heat, upon which the temperature of the sample increases from…

A: Formula, Q = MSΔT

Q: You have a piece of iron, the specific heat of iron, the specific heat of iron is 0.449 J/g °C and…

A: Specific heat :-  The amount of heat required to rise the temperature of one gram of a substance…

Q: How much heat energy is lost when a 15.00 gram sample of water cools from 42°C to a final…

A: Specific heat capacity is defined as the heat  required to raise the temperature of one gram of a…

Q: A 40 g sample of water is raised 10oC, with water having a specific heat of 4.184 J/g*C, what amount…

A: Specific heat capacity: The quantity of heat energy required to raise the temperature of one gram of…

Q: 22.0 g of a metal absorbs 713 J when it is heated from 28.3 degrees to 72.8 degrees what is the…

A:

Q: If 2500 cal of heat are absorbed by 150 grams of water that is initially at 23°C, what is the…

A: Given, mass of water = 150 g  Initial Temperature , Ti = 23°C  Tf = ?  Heat absorbed = 2500 Cal

Q: 2. When 39.0 grams of silver are cooled from 80.0°C to 63.0°C, 159 joules of heat are released.…

A: Specific heat:The amount of heat required to increases the temperature of the 1 g of the substance…

Q: Ethanol and gold each absorb the same amount of heat energy at room temperature. If ethanol has a…

A: As we know, amount of heat added is expressed as Q= mc ∆t Where Q=Amount of Head Added c =Specific…

Q: An iron nail with a mass of 12g absorbs 17 J of heat. If the nail was initially at 30 °C, what is…

A:

Q: How do I calculate the specific heat of metal if 1027 joules of energy are needed to raise the…

A: q = m .C . ΔT  WHERE  heat = q = 1027 J  mass of metal = m = 42.9 g specific heat of metal  = C =…

Q: how many kilojoules of heat will be relesed when exactly 0.5 mole of iron is heated from 28.0…

A: No. of moles of Iron = 0.5 mole Molar mass of Iron = 55.845 g/mole So, mass of Iron  = No. of moles…

Q: A sample of water of unknown mass undergoes a temperature change from 68.09°C to 72.61°C with a…

A: Given, a sample of water of unknown mass. undergoes a temperature change from 68.09°C to 72.61°Cwith…

Q: If 125 cal of heat is applied to a 60.0-g piece of copper at 24.0 C, what will the final temperature…

A: The amount of heat required to raise the temperature of the sample is obtained by multiplying the…

Q: Calculate the change in the internal energy for a certain process if 800 J of work is done on the…

A:

Q: 24. In the specific heat equation, what unit must temperature be? Fahrenheit Kelvin Joules Celsius

A: We know , Specific heat equation is ; q = m × C × ∆T  q = heat Absorbed or released m = mass of…

Q: a 155.0g piece of copper at 117 degrees celcius is dropped into 250.0g of water at 16.5 degrees…

A: Use calorimetry principle to get answer Heat flow from high temperature to low temperature. Heat=…

Q: A home swimming pool contains 165 m3 of water. At the beginning of the swimming season, the water…

A: The amount of heat required is determined by using formula q= m c delta T

Q: How much heat has to be added to 528 g of copper at 22.3°C to raise the temperature of the copper to…

A: Specific heat is defined as the amount of  heat  required to raise the temperature of 1g  substance…

Q: What will be the temperature change of the metal?

A: q = mc∆T  q is the amount of heat energy required  m is the mass of substance  c is the specific…

Q: What is the temperature change on a 75.0 g sample of mercury?

A: q = mc∆T  q is the amount of heat energy absorbed m is the mass of sample c is the specific heat  of…

Q: The initial temperature of a 12g sample of copper is 25 C.  If the sample absorbs 226J of heat, what…

A: Given: Heat absorbs = 226 J Heat capacity of copper = 0.385 J/g⋅∘C Mass of copper = 12 g Initial…

Q: If we add 30.0 J of heat to 10.0 grams of aluminum, by how much will its temperature increase? The…

A:

Q: It is determined that a block of metal absorbed a 125.5 J after undergoing a temperature change from…

A:

Q: A sample of water with a mass of 662.8 g undergoes a temperature change from 81.40°C to 18.91°C what…

A:

Q: heat capacity

A:

Q: 8. What is the mass of a sample of glass (specific heat = 0.50 J/g°C), if it requires 490 J of heat…

A: The question is based on the concept of chemical thermodynamics. It involves calculation of the mass…

Q: The specific heat of an unknown metal is calculated to be 3.74J/g*c. What is the mass of the sample…

A: Specific heat :-  The amount of heat required to rise the temperature of one gram of a substance…

Q: calculate the heat lose (in Joules) by 115 g of water as it cools from 71.4 C to 34.4 C

A: Given data, Mass of water = 115 g Initial temperature = 71.4oC Final temperature = 34.4oC

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.