A 228-g coin made of zinc is heated and placed in 100.0 g of water at 16.0°C. The temperature when the zinc and water come to thermal equilibrium is 24.0°C. What was the initial temperature of the zinc coin? Cs(Zn) = 0.389 J/g·K, Cs(H2O) = 4.18 J/g·K Express your answer to one decimal place.   T1 of coin = Answer °C

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 216.0 g sample…

A: The mass of the sample is = 216.0 g The increase in the temperature is = 19.1 - 1.3 = 17.8oC = 17.8…

Q: Calculate the heat that must be supplied to a 500.0 g stainless steel vessel containing 450.0 g of…

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

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 643.0 mg sample…

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Q: The specific heats of some common substances are as follows: iron = 450 J/(kg ·°C) sand = 830 J/(kg…

A: The given specific heat values are,

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 480.0 mg sample…

A: Given: Mass of mercury=480.0 mg=0.4800 g Temperature change, ∆T=(48.8+273)-(35.2+273)=13.6 K Heat…

Q: The nutritional information label for food items provides the calorie content and other nutritional…

A: Given: Donuts Composition:  Carbs = 32 g Fats = 12 g Proteins = 2g and Energy Value: Carbs = 17 KJ/g…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 182.0 mg sample…

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Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 796.0 mg sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 186.0 mg sample…

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Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 674.0 mg sample…

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Q: A ball bearing at 220. degrees C is dropped into 250. g of water. The water warms from 25.0 to 30.0…

A: When temperature of any specified substance gets raised by 1 degree, the heat change is recognized…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.53 kg sample…

A: We know that  Q = m*s*ΔT        ----------(1) Where, Q is heat energy               m is mass of…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 320.0 mg sample…

A: Consider the given information is as follows; Heat needed (q) = +3.51 JMass of the sample = 320.0 mg…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.91kg sample…

A: Given: mass of substance = 1.91 kg = 1910 g Temperature change = 0.6°C to 15.5°C Heat needed = 3.96…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.87 kg sample…

A:

Q: In order to change the temperature of 147 g of lead from 22 o C to 55.oC, how many Joules are…

A: Q = mc∆T Q = heat M = mass C = specific heat capacity ∆T = change in Temp.   M = 147 g ∆T = Tfinal –…

Q: An electric range burner weighing 610.0 grams is turned off after reaching a temperature of 483.5°C,…

A: Heat loss = Heat gain  ( mS∆T )burner = ( mS∆T ) water

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 590.0 g sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 236.0 mg sample…

A: We know that q = mc∆T ....(1)  q = heat required = 3.7 J, ∆T = increase in temperature = 11.6 °C…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 282.0 g sample…

A: We know that , amount of heat (Q) -  Q = m.s.∆t

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 198.0 mg sample…

A: Each chemical reaction is associated with the liberation or intake of a certain quantity of heat.…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 748.0 mg sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.25 kg sample…

A:

Q: hemist carefully measures the amount of heat needed to raise the temperature of a 886.0 mg sample of…

A: Specific heat capacity is amount of heat needed to increase one gram of substance by one degree

Q: A block of copper is heated to 392 °C and then is dropped into a coffee cup calorimeter containing…

A: Heat gained by water = Heat lost by block of copper Therefore,  qwater = -qcopper   Heat gained by…

Q: A metal radiator is made from 13.96 kg of iron. The specific heat of iron is 0.449 J/g °C. How much…

A: Given;

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 162.0 g sample…

A: Answer: When heat is added to a substance, its temperature rises but the value of temperature rise…

Q: In the laboratory a student determines the specific heat of a metal. He heats 18.8 grams of aluminum…

A: Given that-Mass of aluminium=18.8 gramsIts initial temperature=98.63°CMass of water=79.1 gramsIts…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 206.0mg sample…

A: Given : Mass of sample = 206 mg = 0.206 g…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 663.0 mg sample…

A: Given Mass = 663 mg = 663 x 10-3 g Heat = 12.8 J T1 = 0°C T2 = 21.4°C

Q: 3) Calculate the heat capacity of a piece of wood if 1500.0 g of the wood absorbs 6.75x104 joules of…

A:

Q: A metal radiator is made from 25.07 kg of iron. The specific heat of iron is 0.449 J/g °C. How much…

A: The mass of iron metal is = 25.07 kg The heat capacity of iron metal is = 0.449 J/goC Increase in…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 228.0 mg sample…

A: The formula to calculate heat is as follows: Q= ms∆T Q is heat released/absorbed. m is mass of the…

Q: A beaker of hot water with a volume of 43.9 mL has an initial temperature of 94.3 °C. You place a…

A:

Q: A 1.37 g sample of butane, C4H10(g), was burned in a bomb calorimeter in the presence of excess…

A: Mass of butane = 1.37 g Initial temperature = 23.6°C Final temperature = 35.6°C Heat capacity of…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 794.0 g sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.75 kg sample…

A: Given: Mass of sample = 1.75 kg Initial temperature = 22.2oC Final temperature = 45.4oC Heat…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 614.0 mg sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.26 kg sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.61 kg sample…

A: We have to calculate the specific heat.

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.37kg sample…

A: Mass of the sample is 0.37 kg and the temperature is raised from – 1.2 oC to 14.5 oC. The heat…

Q: 1. How much heat must your body transfer to 500.0g of water to heat it from 25.0°C to body…

A:

Q: A 43.9 g spoon made of pure silver (c = 0.235 J/g C) at 20.1 celcius is used to stir an 8 oz. (240…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 833.0 mg sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 309.0 g sample…

A: Given: The mass of the given sample, (m) = 309 g. The initial temperature, (T1) = -2.9 0C=…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 284.0 mg sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.57 kg sample…

A:

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.46 kg sample…

A: Specific heat--->> The specific heat capacity of a substance is the amount of energy required…

Q: A 15.0-mL sample of benzene at 21.3 °C was cooled to its melting point, 5.5 °C, and then frozen. How…

A: Given, density of benzene = 0.80 g/mL Volume of the solution = 15.0 mL  Mass of benzene = Density x…