A silver block, initially at 58.5 °C, is submerged into 100.0 g of water at 24.8 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.2 °C. What is the mass of the silver block?

A hot lump of 25.4 g of aluminum at an initial temperature of 83.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.

A 1095 g piece of iron initially at 1371 °C is submerged in 1000.0 g of water initially at 20.0 °C. The temperature of the water increases, and some of the water evaporates. At thermal equilibrium, the final temperature of the iron, water, and water vapor (steam) is 100.0 °C. How many moles of water evaporated to reach thermal equilibrium? The specific heat capacity of iron is Cs, Fe = 0.449 J /g.°C The specific heat capacity of liquid water is Cs, water = 4.18 J/g.°C The enthalpy of vaporization of water is AHvap :40.7 kJ/mol Circle your answer on the written template. Be sure that it is in the correct units (mol) and has the correct number of significant figures.

A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 1.44 g of CaClh(s) are dissolved in 104.80 g of water, the temperature of the solution increases from 24.43 to 26.88 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CaCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol

A 395.7 g sample of water at 20.0 °C is mixed with 100.0 g of a certain metal at 95.0 °C. After thermal equilibrium was established, the temperature of the mixture is 24.6 °C. What is the specific heat capacity of the metal?

A sheet of gold weighing 10.0 g and at a temperature of 18.0°C is placed flat on a sheet of iron weighing 20.0 g and at a temperature of 55.6°C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. (Hint: The heat gained by the gold must be equal to the heat lost by the iron.

A 350.0 g iron pot is heated on a stove for a period of time until it is hot. The stove is turned off and 516 g of cold water (10.0 °C) is added to the pot. When thermal equilibrium is reached, the temperature of the water is  28.4 ° C. What was the initial temperature of the iron pot, assuming heat was exchanged between these two objects and none was lost to the surroundings? (The specific heat capacity of iron is 0.450 J/g °C. The specific heat capacity of water is 4.184 J/g °C) Give only the numerical answer in the box and not units. Give 4 sig figs in your answer. Show the calculations for the problem by writing it on a paper, upload the image file/pdf file in the question for file upload.

Explain the difference between heat capacity and specific heat of a substance. Heat capacity refers to the heat required to raise the temperature of a substance by 1 °C; specific heat refers to the heat required to raise the temperature of 1 gram of a substance by 1 °C. Thus, heat capacity is an intensive property, and specific heat is an extensive one. Specific heat refers to the heat required to raise the temperature of a substance by 1 °C; heat capacity refers to the heat required to raise the temperature of 1 gram of a substance by 1 °C. Thus, heat capacity is an intensive property, and specific heat is an extensive one. Heat capacity refers to the heat required to raise the temperature of a substance by 1 °C; specific heat refers to the heat required to raise the temperature of 1 gram of a substance by 1 °C. Thus, heat capacity is an extensive property, and specific heat is an intensive one.

A 32.5-g iron rod, initially at 22.7 °C, is submerged into an unknown mass of water at 63.2 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.5 °C. What is the mass of the water?