1. Determine the amount of energy required to melt 15.0 grams of ice. 2a. If a 2000g block of metal LOST 3120 J of heat energy as it cooled from 212 degrees C to 200 degrees C, what is the specific heat of the metal 2b. What is the element ?

Q: If 50.0 g of water at 25.0 °C absorbs 14.5 kJ of heat, what is the final temperature of the water?…

A: Given  q = 14.5 kJ = 14500 J C = 4.184 J/g.°C Ti = 25°C Tf = ?

Q: A piece of silver, with specific heat capacity of 0.235 J/(g.°C), is added to an insulated container…

A: Given: The specific heat of water, (cH2O) =4.184 J(g. 0C). The specific heat of silver, (cAg) =…

Q: A sample of aluminum absorbs 11.2 J of heat and its temperature increased from 23.2°C to 57.5°C.…

A: We know that heat absorbed  by Al  q = m*s*ΔT where q = heat absorbed  by Al; m= mass of Al; s =…

Q: The temperature of a 5.0 g sample of Aluminum increases from 25°C to 30°C. How many joules of heat…

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Q: The specific heat of a certain type of cooking oil is 1.75 J/ (g.°C). How much heat energy is needed…

A: We have to predict the energy needed.

Q: How much energy would it take to heat a section of the copper tubing that weighs about 725.0 g, form…

A: The mass of the copper tube is = 725.0 g Raise in temperature is = 22.6-15.01 = 7.59oC The heat…

Q: A 500 g piece of iron (CP = 25.09 J/(mol · °C) changes 7°C when heat is added.  How much heat energy…

A: Given mass of iron = 500 g Molar mass of iron = 55.85 g/mol Number of moles of iron = 500/55.85 =…

Q: Heated bricks or blocks of iron were used long ago to warm beds.  A 1.49-kg block of iron heated to…

A: Given, mass of iron block =1.49 kg =1.49×103 ginitial temperature Ti =155 °Cfinal temperature Tf =22…

Q: The evaporation of water is endothermic:         H2O(l)  + 44.01 kJ   -------->   H2O(g)       If…

A: Endothermic reaction is a reaction in which heat is absorbed.

Q: How many grams of water can be heated from 26.1°C to 38.4°C by the heat released from 80.8 g of…

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Q: Consider the following data: When metals A and B are placed in contact with each other, which of the…

A: Answer is Option (B)

Q: How much heat is required to warm 1.50 L of water from 25.0°Cto 100.0°C? (Assume a density of 1.00…

A: We can solve this problem by using the following relation: q=m×c×△T Where: q=Heatc=specific heat(…

Q: The evaporation of water is endothermic H2O(l)+44.01kj------>H2O(g) If 275kj of heat is absorbed,…

A: Given reaction,      H2O(l) + 44.01kj → H2O(g)   Calculate the moles of H2O evaporated,         275…

Q: How much energy must be removed from 13.7 grams of gaseous helium in order to decrease the…

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Q: A 44.3 g sample of water at 100.00 °C (specific heat of water = 4.184J/g.°C) was placed in an…

A:

Q: When 45 g of an alloy metal, at 25°C, is dropped into 100.0 g of water, the alloy absorbs 956 J of…

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

Q: 500 g piece of iron changes 7°C when heat is added. How much heat energy produced this change in…

A: Given that: Mass of iron(m) = 500g Change in temp(dT) = 7°C Specific heat of iron(C) = 0.444J/g°C

Q: 5. A 295 g sample of unknown metal is at an initial temperature of 13.00 °C absorbs 75.0 kJ. The…

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Q: How much heat is required to warm 28 g of iron from 12°C to 84° C?. Specific heat of iron is 0.444…

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Q: Evaporating sweat cools the body because evaporation is an endothermic process:H2O(l)…

A: Evaporation: The process in which liquid convert into vapor or gaseous form is called evaporation.…

Q: A piece of unknown substance weighs 44.7 g and requires 2110 J to increase its temperature from…

A:

Q: 9. A piece of aluminum is heated to a temp of 71.8°C, then placed in 150.0 mL of water at 20.7°C…

A: Given data, For Aluminum, Cp =0.903 J g-1 ℃-1 mass m=? T1=71.8 ℃  T2=25.6 ℃

Q: A 248.5 g water bath is heated to 98.2 ˚C from 22.2 ˚C.  How much heat was absorbed by the water, in…

A: Specific heat and heat of the Substance are interrelated with each other by -   Q = C m ∆T Here, Q =…

Q: To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of…

A:

Q: 11. What is the specific heat of carbon tetrachloride (CCL) if it requires 77 J of heat to raise the…

A:

Q: Question attached

A: Given : Mass of water = 35.5 g Mass of metal = 9.323 g Initial temperature of water = 19.42 oC Final…

Q: Calculate the total heat energy in joules needed to convert 20.0g of water from 30.0 c to -20.0c

A: q = mc∆T            m = mass  of water = 20.0 g             c = 4.184 J/g. oC…

Q: metal is heated from 25.0°C to 250.°C, and was found to have absorbed 878 J of energy as heat. What…

A: Heat flow from high temperature to low temperature.

Q: beaker contained 69.68 g of water at 15.25°C. A 81.2-g sample of metal at 52.22°C was placed in it,…

A:

Q: 1.)  How much energy is required to raise the temperature of 10.7 grams of solid zinc from 20.3°C…

A:

Q: How much heat energy is required to raise the temperature of 0.366 kg of copper from 23.0 C to 60 C?…

A: The mass of copper is = 0.366 kg The raise in temperature is = 60-23 = 37oC The heat capacity of…

Q: 10. How much heat is required to bring the temperature of one kilogram of aluminum from 20-C to…

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

Q: How much heat has to be added to 513 g of copper at 22.3°C to raise the temperature of the copper to…

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Q: A 28.602 g sample of a metal is heated to 99.9°C in a hot water bath until thermal equilibrium is…

A: Let c be the specific heat of the metal Heat lost by the metal = mass x specific heat x temperature…

Q: 1.3. A copper cylinder has a mass of 65.5 g and a specific heat of 0.092 cal/g.°C. It is heated to…

A: Answer 1.3 mass of copper cylinder = 65.5 g specific heat of copper cylinder = 0.092 cal/g.0C…

Q: A 25.0 g mercury is heated from 25 °C to 155 °C and absorbs 455 J of heat in the process. What is…

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

Q: A metal object with mass of 20.9 g is heated to 97.0 °C and then transferred to an insulated…

A:

Q: 559.4 J of heat was added to 8.00 g of water. The final temperature of the water was measured as…

A: Given: Heat Energy (Q)= 559.4 J Mass of water (m)= 8.00 g Final Temperature (T2) = 64.2 0C Specific…

Q: What is the change in temperature of a 13.6 g sample of water that absorbs 1,524 J of heat?

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

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: A 100 g sample of each of the following metals is heated from 35 °C  to 45 °C. Which metal absorbs…

A: Given information, Metal       Specific Heat Capacity (J/gž°C) Copper    = 0.385 Mercury  = 0.138…

Q: 2. A 25.0 g bold made of an alloy absorbed 250 J of heat as its temperature changed from 25.0 °C to…

A: Applying formula Q= mc∆t

Q: A 25.0 g sample of lead, specific heat = 0.128 J/g  degrees Celcius , was warmed from 35.0 derees…

A: Heat absorbed by lead is calculated as follows,

Q: The specific heat of a certain type of cooking oil is 1.75 J/(g.°C). How much heat energy is needed…

A: We have to calculate the heat required.

Q: The specific heat of a certain type of cooking oil is 1.75 J/(g⋅°C).1.75 J/(g⋅°C). How much heat…

A: Given: The specific heat, ‘c’ of cooking oil is 1.75 J/(goC) Mass, ‘m’ of oil is 2.42 kg Initial…

Q: 3. How much heat is required to rise the temperature of 0.5 kg water from 30°C to its boiling point?…

A: Question 3. Given that, the mass of water is m = 0.5 kg. The initial temperature is T1 = 30oC =…

Q: A 4.8 sample of water starting 56 C loses 448 J of energy in the form of heat. What is the final…

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Q: A sample of 175°C copper is placed into a beaker with 100 grams of 25°C water. Which sample of…

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Q: A 113.0 gram gold bar was heated in an experiment and 3,000 J of energy was transferred to the bar.…

A: