The heat content of 93 g of water at 100°C cooling to 37°C is The heat released when 93 g of water vapor at 100°C cools to 37°C is kJ.

Q: What quantity of energy, in joules, is evolved when 1.00 mol of liquid ammonia cools from -33.3…

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Q: Suppose that 1.11 g of rubbing alcohol (C3H8O)evaporates from a 70.0 g aluminum block. Aluminum has…

A: This question requires manipulation of units. At first, calculate the no. of moles of rubbing…

Q: If 27.5 g of MgCl₂ are dissolved 500.0 g of water at 20.0 °C in an insulated container, a…

A: Given that, The mass of the MgCl2 is 27.5 g. The mass of the water is 500.0 g. So, the total mass of…

Q: Steam can cause more severe burns than water, even if both are at the same temperature. Calculate…

A: Steam must release energy equivalent to the enthalpy of vaporization of water to convert to water.…

Q: A sample of lead is heated to 189.4oC.  It is then placed in a cup containing 32.8 g water at…

A: The relationship between heat , specific heat capacity and change in temperature is given by the…

Q: Benzene (C6H6) is an organic compound that boils at 80.1°C. If 100.0 grams of liquid benzene at…

A: The heat of Vapourisation is the amount of energy that must be added to the liquid substance to…

Q: 0.810-g piece of lithium metal is dropped into a mixture of 50.0 g ater and 50.0 g ice, both at 0°C.…

A: The moles of Li can be calculated as,mass of lithium, Li = 0.870 gMolar mass of Li= 6.941 g/molMoles…

Q: A piece of calcite is heated to 72.0°C and placed in a styrofoam coffee cup containing 25.0 mL of…

A: GIVEN: The temperature of Calcite=72.0°C Volume of water= 25.0 mL The initial temperature of water=…

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…

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Q: Calculate the amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol…

A: Given: Mass of ethanol = 79.0 g Initial temperature = 198.0 K=-75.150C Final temperature = 285.0 K…

Q: Suppose that 1.15 g of rubbing alcohol (propan-2-ol) evaporates from a 65.0 g aluminum block. If…

A: Given, Mass of alcohol evaporate = 1.15 g Mass of Aluminum block = 65.0 g Initial heat of the block…

Q: kJ of heat were added? Specific heat 34 J/g°C. 1 calorie = 4.184 J %3D

A: Heat  (q) = 36.5 ×1000 = 36500 J Mass of water = 275 g Heat capacity (s) = 4.184 J/g-°c Heat (q) =…

Q: How much heat (in kJ) is needed to raise the temperature of 100.0 grams of water by 25.0 °C?  The…

A: Mass of water(m) = 100 gm  specific heat capacity of water(s) = 4.184 J/g·°C  Increase in…

Q: The specific heat capacities of copper, gold, and cobalt are given. Based on this information, which…

A: Specific heat capacity means the amount of heat required to raise the temperature of 1 gram of a…

Q: Calculate the amount of heat energy (in joules) released to DROP the temperature of 30.0 g of water…

A: The specific heat of a substance is defined as the amount of heat required for raising the…

Q: If a 125 g sample of iron is heated to 250.0oC and then placed in 500.0 g of water at 25.0 oC in an…

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Q: If 40.0 g of hot water at 80.0oC is added to 60.0 g of cold water at 20.0oC, what is the final…

A: The final temperature is 44 oC

Q: If a 125 g sample of iron is heated to 250.0oC and then placed in 500.0 g of water at 25.0 oC in an…

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Q: A 3.75 g piece of gold initially at 587.15 K is dropped into 20.6 mL of water at 295.75 K. Calculate…

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Q: Substance Specific Heat, c (J/g×°C) Water 4.184 Granite 0.803 Mercury 0.140 Silver 0.235 Aluminum…

A: Heat given by Aluminum = heat taken by water

Q: A 325.0 g piece of gold at 427.0 °C is dropped into 200.0 mL of water at 22.0 °C. The specific heat…

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

Q: How much heat is liberated (in kJ) from 2.57E2 g of silver when it cools from 8.2E1 °C to 2.67E1 °C?…

A: We have to predict the heat released.

Q: When 1 mol of CS2 (I) forms from its elements at 1 atm and 25.0°C, 89.7 kJ of heat is absorbed. It…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: Silicon, used in computer chips, has a heat capacity of 0.712 J·g-1·°C-1. If  500  J of heat is…

A: Given: Heat capacity of silicon = 0.712 J g-1 °C-1 Absorbed heat = 500 J Mass of silicon = 8.13 g…

Q: What quantity of heat (in kJ) will be absorbed by a 69.5 g piece of aluminum (specific heat = 0.930…

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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: 12.755 g of a metal initially at 99.0ºC are placed into 75.0 g of water intially at 23.0ºC. The…

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Q: Calculate the amount of heat (in KJ) required to raise the temperature of a 86.0g sample of ethanol…

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Q: Calculate the heat absorbed when 149 g of liquid ethanol at 25.0°C is converted to gaseous ethanol…

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Q: Dissolving 3.0g of CaCl2 in 150.0g of water in a calorimeter at 22.4oC causes the temperature to…

A: Given,  Mass of CaCl2 = 3 g  Molar mass of CaCl2 = 110.98 g/mol Mass of Water, m = 150 g  Initial…

Q: substance is initially at 20.3 ∘C.20.3 ∘C. After absorbing 2063 J2063 J of heat, the temperature of…

A: Heat of reaction is difference of energy of product  and energy of Reactant. If heat of reaction is…

Q: How much heat is released when the temperature of an 8.21 g sample of gold decreases from 87.9 oC to…

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

Q: If 29.00 g of aluminum at 76.45 °C is dropped into 125.7 g of water at 34.04 °C, what will be the…

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Q: Calculate the amount of heat, in Joules, needed to raise 34.0g of water from 55.0°C to 76.0°C. The…

A: Here we are required to find the amount of heat needed to raise 34.0g of water from 55.0°C to 76.0°C…

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 student conducted several calorimetry investigations. In the first of the investigations, the…

A: Mass of metal piece Mm = 21 g  Temperature of metal piece Tm = 80°C Specific heat capacity of metal…

Q: When a 43.0 g sample of metal at 100.0 oC is added to 38.0 g of water at 23.72 oC, the final…

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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 232 mL soft drink (that contains mostly water) initially at 11.0 °C is cooled by adding 156.3 g of…

A: A 232 mL soft drink (that contains mostly water) initially at 11.0 °C is cooled by adding 156.3 g of…

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

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Q: Calculate the total energy in kJ required to change the temperature of 591 g water from 96.0  oC to…

A: The process of cooling water from  96.0  oC to -111 oC will have below steps. 1) cooling hot water…

Q: Water exists as a liquid at room temperature (25.0°C). If 300 kJ of heat energy is added to 100 g…

A: Answer:Increasing the temperature of liquid water up to its boiling pointVaporization of…

Q: heat of vaporization (kJ/mol) of methanol.

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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…