What mass of water

Q: Calculate the amount of heat (in kJ) required to raise the temperature of 1.65 lb of water from 294K…

A: Given : Initial temperature =  294K Final temperature =  303K Mass of water = 1.65lb

Q: a lab, there was a student who finds it takes 62.8J to increase the temperature 12.9g of solid iron…

A: In given question  Heat = mass × specific heat × change in temperature  Used

Q: mestion 41 of 41 Suppose a boil water notice is sent out advising all residents in the area to boil…

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Q: A 4.22 kg piece of copper metal is heated from 20.5°C to 224.5°C. Calculate the heat absorbed (in…

A: The mass of 1.0 kg in g is 1000 g. The mass of the 6.22 kg copper in g is 6220 g. 1000 g=1.0 kg 4.22…

Q: How many milliliters of water at 21 °C with a density of 1.00 g/mL must be mixed with 220 mL of…

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

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Q: How much heat did a cold water sample absorb if 53.88ml of water initially at 22.2 celcius to 32.5…

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Q: mass

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Q: What is the specific heat capacity of an 872 g sample that requires 3.18×104 J of heat to increase…

A: Given data:- Mass(m) = 872g = 0.872Kg(1kg = 1000g)Heat(q) = 3.18×104J Initial Temperature (Ti) =…

Q: The specific heat of a certain type of oil is 1.89 J/g°C. How much heat energy is needed to raise…

A: The amount of heat required is related to specific heat capacity as,…

Q: A 31.1 g wafer of pure gold at 69.3 is submerged into 64.2 g of water at 27.8 in an insulated…

A: given: mass of gold = 31.3 g initial temperature of gold = 69.3oC mass of water = 64.2 g initial…

Q: L00 g of wate

A: Specific heat tells us that how much heat is needed to increase the temperature of 1 g of that…

Q: How much heat must be added to a 8.21 g sample of gold to increase its temperature from 25 oC to…

A: We know that Q = m×C×∆T Q = heat m = mass C = Specific heat ∆T = change in temperature m = 8.21g C =…

Q: neat re

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Q: in the laboratory a student finds that it takes 47.8 Joules to increase the temperature of 11.2…

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

Q: How much heat is required to convert solid ice with a mass of 960 g at a temperature of -10.0 °C to…

A: Heat in kilojoules can be calculated using the specific heat capacity, temperature difference and…

Q: A calorimeter contains 2.50 kg g of water at 37.0 °C. A 225-g sample of ice (at -20.0 °C) is added…

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Q: A 35.0-g sample of water at 25°C is mixed with 45.0 g of water at 88°C. Calculate the final…

A: Calculate for the final temperature of the mixture see step-2 for further Calculation and concept…

Q: You add 100.0 g of water at 58.3 °C to 100.0 g of ice at 0.00 °C. Some of the ice melts and cools…

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Q: The temperature of a beaker containing 194 mL (density of water is 1 g/mL) of water changes from 16…

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Q: student is asked to determine the heat of solution in J/g for the compound ammonium nitrate…

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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 solution is made by mixing 197.3 g of ethanol initially at 10.5°C with 250.0 g of water initially…

A: We know that, according to the law of conservation of heat energy, energy gained or loss by the…

Q: gold bar of  unknown amount absorbs 1.09 kJ of heat and raises its temperature from 5.3 °C to 72.2…

A: Heat absorbed, q = mCs∆T  ∆T = T2 - T1  T1 = Initial temperature T2 = Final temperature m = Mass of…

Q: For this question, you are trying to determine which beaker will have more heat absorbed and why.…

A: Answer:- This question is answered by using the simple concept of calculation of heat absorbed by…

Q: The specific heat of mercury is 0.140 J/g°C. Calculate the heat necessary to raise the temperature…

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Q: a) A person drinks four glasses of cold water (3.0°C) every day. The volume of each glass…

A: Given: volume=2.6×102 mLInitial temperature=3.0oCFinal temperature=37oC To find: Heat supplied

Q: 79.8 grams of a metal that is at temperature 92.39 oC is placed in 186.3 mL of water at 19.79 oC.…

A: Here use thermal equilibrium concept. Here final temperature is 24.68 degree celcius, So metal…

Q: Determine the final temperature of a gold nugget (mass = 376 g) that starts at 288 K and loses 4.85…

A: Specific Heat Capacity of gold is =0.128 J/gc Initial temperature = T1 = 288K…

Q: A 15.0-mL sample of benzene at 21.0 °C was cooled to its melting point, 5.5 °C, and then frozen. How…

A: Calculate the mass of benzene from density,

Q: Suppose a boil water notice is sent out advising all residents in the area to boil their water…

A: Given: The volume of water, (VH2O) = 12 L = 12000 mL. The initial temperature of the water, (T1) =…

Q: How much heat, in joules, must be added to a 95.8 g iron block with a specific heat of 0.509 J/g °C…

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Q: What quantity of heat (in kJ) will be absorbed by a 78.3 g piece of aluminum (specific heat = 0.930…

A: We have to calculate the heat absorbed by aluminium

Q: How much heat, in calories, must be added to a 102.0g iron block with a specific heat of 0.449 J/g…

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Q: A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric g…

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Q: A 155.0 g piece of copper at 181 oC is dropped into 250.0 g of water at 17.9 oC. (The specific heat…

A: Assuming the final temperature of mixture is T and specific heat of water = 4.184 J/goC Since the…

Q: piece of metal weighing 50 grams was heated to 100°C and then dropped into 250 grams of  water at…

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Q: Ices] A 21.0 g sample of pure iron at 85 °C is dropped into 66 g of water at 20. °C. What is the…

A: The given problem can be solved by using the formula given below as; mironCiron∆T = mwaterCwater∆T…

Q: In one box of nails, there are 75 iron nails weighing 0.280 lblb . The density of iron is 7.86…

A: Given: Mass of 75 iron nails = 0.280 lb. Specific heat of iron = 0.452 J/g.oC. Since 1 lb = 453.6 g.…

Q: Calculate the amount of heat energy (in joules) needed to raise the temperature of 48.0 g of water…

A: q = m × SH × ∆T  q = heat energy  m = mass of water  SH = specific heat of water  ∆T = change in…

Q: 105 mL of H2 O is initially at room temperature (22.0° C). A chilled steel rod at 2.0° C is placed…

A: The heat lost by water is given by  Q = mw Cw ΔTw  where mw = mass of water = density of water X…

Q: How much heat, in joules (J), must be added to a 75.0-g iron block with a specific heat of 0.449 J/g…

A: Given: Mass of iron block =75.0 g Specific heat of iron =0.449 J/g oC Initial temperature(T1) =25 oC…