Why does water have a high specific heat index? It requires a great amount of energy for water to beco It takes water little energy to get hot. Water changes temperature very easily. P. Water warms up fast when heated by the sun.

Q: 1. Ethanol has a heat of vaporization of +841 J/g when it transitions from liquid to gas What is the…

A: Heat of vaporization is defined as the energy change when one mole of a liquid is converted to one…

Q: How much heat must be absorbed by a 15.0-g sample of water to raise its temperature from 25.0 °C to…

A: The heat absorbed by the given system is determined by using following formula.

Q: Calculate how much heat 32.0 g of water absorbs when it is heated from 25.0°C to 80.0°C. Specific…

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Q: How much heat is absorbed when 32.6 g of H20 (1) at 100°C is converted to vapor at 100°C? Note: 1…

A: Number of moles = Mass/molar mass Heat absorbed = Number of moles x molar heat of vaporization

Q: 24. Liquid water has a specific heat capacity of 4.18 Jig °C. For water, AH, at its boiling point is…

A: In the case of water, 4184 J of energy is absorbed which is also equals to 1 calorie of energy to…

Q: A man ate 0.50 pound of cheese (an energy intake of 4 × 103 kJ). Suppose that none of the energy was…

A: Given data, Energy = 4 × 103 kJ The enthalpy vaporization = 44.0 kJ The molar mass of water =…

Q: If substance X has a higher specific heat value, how will the temperature of substance X compare to…

A: Given, The substance X has higher specific heat than…

Q: The enthalpy for boiling water is 40.7 kJ/mol. How much heat is required to boil 1105.1 g of water?

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Q: An arctic explorer is trying to create drinking water by converting an ice ball into liquid. The ice…

A: Given that : The mass of ice = 225 g The initial temperature of ice = -23°C The final temperature of…

Q: Which of the following statements is true? Specific heat capacity is dependent on the amount of the…

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Q: 1. Compare the change in temperature values for your data of water compared to the metal in part A.…

A: As per bartleby guidelines, I am allowed to answer one question at a time. Please reupload the rest.…

Q: Based on the thermodynamic properties provided for water, determine the amount of energy released…

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Q: How much heat is required to raise the temperature of 789g of liquid ammonia, form 25°C to 82.2°C?

A: Given: The mass of liquid ammonia is 789 g. The initial temperature is 25oC. The final temperature…

Q: How much heat energy is needed to warm 50.0 g of carbon (specific heat = 0.71 J/g ºC) from 25 ºC to…

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Q: 23.  Calculate the mass of water in grams that can be heated from 0 oC to 15 oC by the amount of…

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

Q: What change in energy is required to heat 55.00 g of water at 15.00 degrees C to vapor at 180.0…

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Q: A 36.62 g sample of a substance is initially at 24.8 °C. After absorbing 1921 Jof heat, the…

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Q: How much heat is absorbed when 25.0g of water warms from 10.2oC to 38.0oC

A: According to calorimetry,  q = m × c × ∆T Where q = heat released or heat absorbed,   c = specific…

Q: How much heat (in kJ) would be required to convert 21.0 g of ice to water at 0°C?

A: Concept: The branch of chemistry that deals with the structure, properties and the reaction of the…

Q: Two 20.0 g ice cubes at −21.0 ∘C−21.0 ∘C are placed into 265 g265 g of water at 25.0 ∘C.25.0 ∘C.…

A: The heat capacity is the ratio of the energy supplied in the form of heat to the rise in the…

Q: 22) Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the…

A: Two questions based on chemical thermodynamics, which are to be accomplished.

Q: A 51.74 g sample of a substance is initially at 25.6 °C. After absorbing 2939 J of heat, the…

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Q: 7. The temperature of a sample of water increases from 20°C to 46.6°C as it absorbs 5650 calories of…

A: Data given, Heat absorbed, Q = 5650 cal Specific heat of water, C = 1.0 cal/g. °C  Initial…

Q: 6.75 When 1 mol of CS,(I) forms from its elements at 1 atm and 25°C, 89.7 kJ of heat is absorbed,…

A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…

Q: Calculate the amount of heat required to raise the tempature of an 91 g sample of water from 39C to…

A: Given: Specific heat of water = 4.18 J/g⋅∘C. Mass of water = 91 g. Initial temperature (T1) = 39 ∘C…

Q: A 49.12 g sample of a substance is initially at 27.2 °C. After absorbing 1995 J of heat, the…

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Q: A 54.12 g sample of a substance is initially at 25.4 °C. After absorbing 1603 J of heat, the…

A: We know that, Q = mc∆T  Where,  Q = heat  m = mass  c = specific heat  ∆T = change in temperature

Q: 1. Consider the following situation: "A ocean breeze blows over cold ground at night, and fog…

A: A bond is a strong or weak attraction between two atoms in the same environment. The new grouping…

Q: . How much heat must be removed from 15.5 g of water at 90.0°C to cool it to 43.2

A: q=m.c.∆T q= heat  m=mass C.=heat capacity ∆T= difference in temperature

Q: 5. The specific heat of ice is 2.09 J/g°C while the specific heat of lead is 0.128 J/g°C. Explain…

A: Before answering this question let us take some basic idea of specific heat capacity or simply…

Q: A 52.03 g sample of a substance is initially at 28.5 °C. After absorbing 1165 J of heat, the…

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Q: How much energy is needed to convert 64.0 grams of ice at 0.00°C to water at 75.0°C?  Specific heat…

A: Given, Specific heat (ice)= 2.10J/(g°C) Specific heat (water)=4.18J/(g°C) Heat of fusion= 333J/g…

Q: What is the final temperature (in °C) of 500.1 g of water (specific heat = 4.184 J/g.°C) at 24.20°C…

A: q=m×c×(T2-T1) Where  q= heat absorbed m=mass  C=specific heat of the substance T2= final temperature…

Q: What is the final temperature (in °C) of 230.1 g of water (specific heat = 4.184 J/g°C) at 24.20°C…

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Q: A 27.95 g27.95 g sample of a substance is initially at 27.7 °C.27.7 °C. After absorbing 1867 J1867 J…

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Q: How much heat (kJ) is absorbed by 948.0 g of water in order for the temperature to increase from…

A: Specific heat: The amount of heat energy required to raise the temperature of one gram of a…

Q: How much heat is absorbed by liquid water that weighs 550 grams as it is heated from 25C to 95C?

A: Given, mass of water m= 550 g T1=25 ℃  T2=95℃ Cp for water = 4.184 J g-1℃-1 heat q=?

Q: How much heat energy must be removed from 1.2 g of lead (specific heat = 0.128 J/g ºC) to cool it…

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Q: What is the final temperature of 450.1 g of water (specific heat = 4.18 J/g･°C) at 24.2°C that…

A: a Specific heat is  heat is required to increase the temperature of of 1 gram of substance by…

Q: A 413.1 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C.…

A: Given,mass of sample =413.1 gMolar mass of sample = 189.50  g/molTemperature changed = 233.0°C to…

Q: How much heat (in kJ) is required to convert 49.6 grams of butane (C4H10) from an initial…

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Q: What is the final temperature of 420.1 g of water (specific heat = 4.18 J/g･°C) at 24.2°C that…

A: The final temperature of water is to be calculated. 14.00 Normal 0…

Q: What change in energy is required to heat 55.00 g of water at 15.00 0C to vapor at 180.0 0C?

A: The quantity of heat transfers from one form to another is denoted as Q. Given the mass of…

Q: Relate the heat gained by the calorimeter and water with the heat lost by the metal. EXPLAIN

A: The heat gained by the calorimeter or water is always equal to the heat lost by the metal.This the…

Q: A 51.76 g51.76 g sample of a substance is initially at 28.0 °C.28.0 °C. After absorbing 1755 J1755 J…

A: We have mass of sample as 51.76 g , initial temperature as 28°C, heat absorbed as 1755 J, final…

Q: A burning match and a bonfire may have the same temperature, yet you would not sit around a burning…

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Q: How much heat (in kJ) would need to be removed to cool 113.1 g of water from 25.60°C to -10.70°C?…

A: The intermediate steps to cool water from 25.60°C t -10.70°C is represented as:H2O (l, 25.60°C)→H2O…

Q: A 52.76 g sample of a substance is initially at 28.4 °C. After absorbing 1985 J of heat, the…

A: In given question use formula  q = mc∆T  Given : q = 1985 J  m = 52.76 g  ∆T = 133.4 - 28.4 = 105 °C…

Q: 35.19 g sample of a substance is initially at 27.1 °C. After absorbing 1533 J of heat, the…

A: The heat absorbed or released by a substance is guided by its specific heatthe relation between heat…

Q: specific heat

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