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: A patient arrives in the emergency room with a burn caused by steam. Calculate the heat that is…

A: given : mass m = 15 g and 2260 Joules per gram. Hence, 2260 × 15 = 33900 J calculate heat released ?…

Q: Mercury was once used in thermometers and barometers. When 69.7 J of heat are absorbed by 100.0 g of…

A: Given, Heat absorbed Q = 69.7 J change in temperature ΔT = 29.98 - 25 = 4.98 ℃ Mass m = 100 g

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

A:

Q: A 2.0 kg block of aluminum (specific heat capacity = 0.897 J · g¯.°C¯1)at 935 °C is dropped into 1.5…

A: When two substances at different temperatures come in contact, there will be a heat transfer from…

Q: A 100.0-g bar of gold (atomic weight of gold = 196.97 g/mol) is heated from 25 °C to 50 °C during…

A: Given, Mass of Au = 100.0 g  Atomic mass of Au = 196.97 g/mole  Initial temperature = Ti = 25 °C…

Q: One hundred grams of a piece of metal was put in 222.2 g container and the water are at 20 deg C. Cp…

A: Given,  Mass of metal= 100 g Mass of water = 222.2 g  Cp(water) = 4.184 J/g-K Cp(metal) = 0.4444 J/K…

Q: The heat capacity of liquid ethanol is 2.45 J/g-deg C. How much heat do you need to add to 100 g of…

A: Given: Specific heat capacity of ethanol = 2.45 J/g⋅ oC Mass of ethanol = 100.0 g Initial…

Q: How many kJ of heat are necessary to raise the temperature of 10.0kg of liquid water from 24.6C to…

A: Answer           Q = mCvdT given m = 10.0 Kg            m = 10000g…

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: A 42.5 gram piece of chromium is heated to a temperature of 98.70ºC. The metal is then dropped into…

A: Mass of chromium = 42.5 g Mass of water = 36.0 g To find final temperature

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: Consider the following data: When metals A and B are placed in contact with each other, which of the…

A: Answer is Option (B)

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

A: The solution is as follows:

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: 125 g of dry ice (solid CO2) is dropped into a beaker containing 500 g of 66°C water. The dry ice…

A:

Q: Calculate the amount of heat absorbed by 23.0 g of water when its temperature is raised from 31.0°C…

A: Answer

Q: Suppose that 1.01 g of rubbing alcohol (C3H8O) evaporates from a 65.0 g aluminum block. Aluminum has…

A: Given data:

Q: The specific heat capacity of solid iodine is 0.427 J/g⋅⋅oC.  Calculate the final temperature (°C)…

A:

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: How much heat (q) is needed to increased the temperature of 10 grams of water by 15°C? Water…

A: Given: The heat capacity of water, (C) = 4.184 J/g°C The mass of water, (m) = 10 g. The change in…

Q: When 11.55 grams of ammonium nitrate (NH4NO3) are dissolved in 100.0 grams of water at 25.0 °C in an…

A: Given: Mass of NH4NO3 = 11.55 g Mass of water = 100 g Initial temperature = 25oC Final temperature =…

Q: An increase in water temperature is observed when 1.97 g of NaOH is added. The enthalpy change for…

A: Given: The mass of NaOH added = 1.97 g The enthalpy change of the reaction = -2.19 kJ An increase in…

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…

A:

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

A:

Q: Energy in the amount of 460 J is added to a 25.0 g sample of water at a temperature of 15.0 °C. What…

A: we can use the formula:-Q=m·s·∆TQ=Heat addedm=masss=specific heat∆T=(Tf-Ti)=(Final…

Q: If 2.0 KJ of heat energy raises the temperature of a calorimeter containing 45.0 g of water from…

A: 2.0 KJ of heat energy raises the temperature of a calorimeter containing 45.0 g of waterfrom 23.0°C…

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: Determine the enthalpy change when 185 g of water vapor at 121 ° C, undergoes phase changes until it…

A: Number of moles of water vapor = mass/mol.wt. = 185 g/(18.015 g/mol) = 10.2692 mol Given…

Q: Determine the amount of heat energy in joules required to raise the temperature of 7.40g of water…

A: Given:  Mass of water = 7.40 g  Initial temperature = 29°C Final temperature = 46°C Standard data:…

Q: In their Memoir on Heat, published in 1783, Lavoisier andLaplace reported, “The heat necessary to…

A: Given, The specific heat capacity of water is  4.18 J. Initial temperature 0°C. The final…

Q: What is the amount of heat energy in joules required to raise the temperature of 10.00 g water…

A: The required relation is given below.

Q: A 50.0 g block of copper at 90.0 0C is placed in a beaker containing 200.0 g of water at 20.0 0C.…

A: Given,mass of copper = 50.0 gspecific heat of copper = 0.38 J/ (g.K )Initial temperature of copper =…

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: A 46.81 g46.81 g sample of a substance is initially at 25.7 °C.25.7 °C. After absorbing 1415 J1415 J…

A: Given, heat(q) = 1415 J mass(m) = 46.81 g temperature change(ΔT) = Tfinal - Tinitial = 177.9 °C -…

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: Ethanol, C2H5OH, boils at 78.29 °C. How much energy, in joules, is required to raise the temperature…

A: To raise the temperature from 28ₒC to 78.29ₒC, required heat is Q1 = m × c × ∆T   = 4000 g × 2.44 J/…

Q: You add a 5.00 g piece of ice to 25.00g of water at 20 °C. Calculate the temperature of the water…

A: Given: Mass of ice (mi) = 5.00 g Mass of water (mw) = 25.00 g Specific heat of water (Cw) = 4.184…

Q: When 6.72 grams of potassium chlorate (KCIO3) are dissolved in 120.0 grams of water at 25.0 °C in an…

A:

Q: A unknown metal is thought to be gold. When 2.8 J of heat are added to 5.6g of the metal its…

A: Heat given to the metal, Q =2.8 J Mass of metal taken, m =5.6 g Increase in temperature, ∆T = 1.72˚C…

Q: 2Na(s) + 2H₂O(1)→ 2NaOH(aq) + H₂(g) AH = -368 kJ Assuming no heat loss to the surroundings, will the…

A: Introduction :  Enthalpy of fusion can be defined as the change in enthalpy of a substance when a…

Q: A quantity of ice at 0 °C was added to 64.3 g of water in a glass at 55 °C. The final temperature of…

A: Given,Mass of water = 64.3g. Temperature of water = 550C.Final temperature of system = 150C.Heat of…

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

A:

Q: Energy Constants for H2O 334 J/g = Heat of Fusion (Hf) 2260 J/g = Heat of Vaporization (Hv) 2.11…

A: Answer:- This question is answer by using the simple concept of calorimetry which state that heat…

Q: A piece of metal with a mass of 59.047 g was heated to 98.0°C and then put into 100.0g of water…

A: Given: Mass of the metal = 59.047 g The initial temperature of the metal = 98.0 oC The mass of water…