A 135 g sample of H20 at 85°C is cooled. The water loses a total of 15 kJ of energy in the cooling process. What is the final temperature of the water? The specific heat of water is 4.184 J/g-"C. Multiple Choice 27°C 112°C 58°C

Q: The ethylene glycol (d = 1.11 g/mL; c = 2.42) in a car radiator cools from 37.0°C to  25.0°C by…

A: The volume of ethylene glycol is  5468.43 mL

Q: How much energy is required to raise the temperature of 10.8 grams of solid chromium from 21.5…

A: According to thermodynamics: q=mc∆T                  . . . (1) Here, m is the mass = 10.8 g c is the…

Q: A 20.0 g mass of ice is heated from 0°C until it completely turns to vapor at 100°C. If you are…

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Q: A 135 g sample of H2O at 85°C is cooled. The water loses a total of 15 kJ of energy in the cooling…

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Q: Calculate the quantity of heat required to raise the temperature of 60.0 g of water from 22.1 °C to…

A: Specific heat capacity is amount of heat capacity is required to raise temprature of one gram…

Q: How much heat is released when 358 g of water cools from 68.3°C to 18.9°C? The specific heat of…

A: This is the question of thermodynamics Here we have to calculate heat released It uses the formula…

Q: How many total joules of heat does it take to heat up a 3.55 g ice cube at -45.5°C to 35.5°C? g

A:

Q: 6. Water has a specific heat of 4.184 J/g°C while glass (Pyrex) has a specific heat of 0.780 J/g°C.…

A: Specific heat is the amount of heat energy required to raise the temperature of a body per unit of…

Q: - A 2.0 kg piece of aluminum, which is at a temperature of 400 ° C, is cooled   to 50 ° C.   The…

A: Given values -> Weight of aluminium piece = 2.0 kg =2000gm T1= 400°C T2=50°C ∆T = T2-T1 = 50-400…

Q: Q5: A bottle of soda at room temperature 22"C is placed in a refrigerator where the temperature is 7…

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Q: Which of these materials will require the greatest amount of energy to warm from 30 degrees C to 40…

A: Since  the energy required will be proportional to the specific heat of the compounds because  Q =…

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: Specific Heats of Substances Substance Specific Heat (cal/g⋅°C) Brick 0.20 Ethanol 0.58…

A: The concept is based upon specific heat capacity which may be defined as the amount of heat energy…

Q: A 12.42 g of water releases 5239 J of heat. The initial temperature of water is 56.23 degrees…

A: Given data,  Mass of water (m) = 12.42 g  Heat released (q) = 5239 J  Specific heat of water (C) =…

Q: I have 270 mL of hot coffee in an insulated vessel.  I cool it down  to 83 degrees C by adding a 25…

A: If the ice is placed in container with water, the heat start flowing from water to the ice, and…

Q: The specific heat of an unknown liquid is O.32 J/kg K. The density of th liquid is 0.0321 g/ ml. If…

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Q: 1.) In the laboratory a student finds that it takes 4.75 calories to increase the temperature of…

A: 1) Given: Mass of lead = 10.4 g. Amount of heat added = 4.75 calories. The initial temperature of…

Q: A 143-g sample of steam at 100°Cis emitted from a volcano. It condenses, cools, and falls as snow at…

A: Latent heat of fusion : The amount of heat required in order to convert one unit of substance from…

Q: The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the…

A: Below attached file showing the details answer All the best

Q: Ryan is a chemistry student that enjoys hot tea. He wants to determine how much ice is needed to…

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

Q: How much heat in kJ must be added to 175 g of w

A: Specific heat capacity of any material (represented as c) is amount of heat required to raise 1 gram…

Q: Calculate the heat absorbed, in kJ, when 2000. g of water is heated froI 20.0 °C to 99.7°C in an…

A: Heat absorbed by a system cab be calculate by the following formula Q = m×s×[t2-t1] Q = heat…

Q: 8) The addition of 3.31 kJ of heat to a 300. g sample of mercury at 19.0 temperature to rise to 99.0…

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Q: Mercury, with a freezing point of -38.8°C, is the only metal that is liquid at room temperature. How…

A: Given that,  Volume of mercury = 1.60 mL Mass of mercury m = density×volume          = 13.6 × 1.60 g…

Q: A drop of water with a mass of 0.48 g is vaporized at 100 ∘C and condenses on the surface of a 55-g…

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Q: A 115.4 g sample of water absorbs 97.48 kJ of heat. If its initial temperature is 7°C, what will the…

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Q: If 9000.0J of heat are absorbed by 800.0 g of water at 5.0 degree C, what will be its final…

A: Given,  If 9000.0J of heat are absorbed by 800.0 g of water at 5.0  °C, the final temperature of…

Q: The specific heat capacity of liquid mercury is 0.14 J/g°C. How many joules of heat are needed to…

A: Option B is correct. ( 40J )

Q: In the laboratory a student finds that it takes 34.3 Joules to increase the temperature of 13.7…

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Q: 2. How much heat must be removed from 155 g of water to cool it from 92.3 °C to 21.6°C? 16

A: Given that the final temperature is 21.6 degree Celsius and the initial temperature is 92.3 degree…

Q: A yogurt mix is heated in a stainless-steel kettle by steam at 100°C with 90% quality. Steam…

A: It involves two stages .  1) conversion of staem to water  2) then water at 100°C to 80°C  Heat…

Q: How much heat is gained when you raise the temperature of an ice cube that weighs 4.46 grams from…

A: Hence the energy required in each process is given by  1) heating of ice from –4.0 °C to melting…

Q: Calculate the heat lost by a 50.0 g piece of copper metal that decreases it's temperature from 45…

A: Specific heat capacity is the amount of heat that is required to raise the temperature of 1 kg…

Q: 1. How much heat, in joules, is absorbed by 500.0 g of water as its temperature is increased from…

A: So we’ve to calculate the energy and specific heat capacity in the respective question. We can solve…

Q: The temperature of a sample of water increases from 20.0°C to 46.6°C as it absorbs 5650 J of heat.…

A: Given,  Initial temperature = Ti = 20.0 °C Final temperature = Tf = 46.6 °C Amount of heat absorbed…

Q: 100.0 g of 4.0 degrees C water is heated until its temperature is 37 degrees C.Calculate the amount…

A: Heat required = mCsΔT m = Mass of substance Cs = Specific heat of substance ΔT = Temperature…

Q: Q5: A bottle of soda at room temperature 22"C is placed in a refrigerator where the temperature is 7…

A:

Q: Compare the heat given off by 1.0 g of boiling water at 100 °C when it comes in contact with your…

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Q: The freezing point of mercury is -38.8 °C. What quantity of energy, in joules, is released to the…

A:

Q: A 105 g -g sample of steam at 100 °C is emitted from a volcano. It condenses, cools, and falls as…

A: Given : Mass of steam = 105 g Initial temperature of steam = 100 oC And final temperature of water…

Q: heat

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Q: A 50.0 g sample of water at 70.0 °C is mixed with 60.0 g of water at 20.0 °C. Find the final…

A: System is isolated that means No heat is transferred from the system on sorrounding On Mixing of…

Q: The freezing point of mercury is -38.8 degrees Celsius. What Energy is released to the surroundings…

A: using the specific heat capacity and enthalpy of fusion to find the heat released.

Q: In which state (×) does a gram of water loses more heat to cool down to +20 °C?   ___ (l) at +100…

A: 1) Given: Final temperature of water = 20 oC.

Q: A (4.1700x10^1) g sample of water (C = 4.18 J / g ºC) initially is at (5.110x10^1)ºC. What is the…

A: According to the equation, Q=mcdTQ=Heat absorbed or releasedc=specific heat capacitydT=Change in…

Q: Water has a specific heat of 4.18 J/goC. If 35.0 g of water at 98.8oC loses 4.94 kJ of heat, what is…

A: Given, the specific heat of water =4.18 Jg.°Cmass of water =35.0 gramheat lost by system =4.94…

Q: The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to…

A:

Q: A 30.37 g sample of a substance is initially at 28.3 degrees Celsius. After absorbing 2235 J of…

A: The amount of heat (Q) gained or lost by a substance (with mass m) as its temperature changes (ΔT)…

Q: What is the mass of a sample of liquid water that took 35.4 kJ of heat to apply to it to raise its…

A: Answer: option b. 257 g if the mass of a sample of liquid water.

Q: Copper is used in building integrated circuits, chips, and printed circuit boards for computers.…

A: The given data: The heat absorbed by the copper = 228 J The mass of the copper = 125.0 g The initial…