A hot 101.7101.7 g lump of an unknown substance initially at 184.9184.9 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 86.486.4 °C. Substance Specific heat (J/(g·°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 tungsten 0.132 zinc 0.388 water 4.184 Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. a) zinc b) graphite c) titanium d) tungsten e) rhodium f) aluminum

A silver cube with an edge length of 2.36 cm and a gold cube with an edge length of 2.75 cm are both heated to 87.5 ∘C and placed in 105.0 mL of water at 20.2 ∘C . What is the final temperature of the water when thermal equilibrium is reached?   Substance Specific heat (J/g·°C) Density (g/cm3) gold 0.1256 19.3 silver 0.2386 10.5 water 4.184 1.00 A silver cube with an edge length of 2.36 cm and a gold cube with an edge length of 2.75 cm are both heated to 87.5 ∘C and placed in 105.0 mL of water at 20.2 ∘C . What is the final temperature of the water when thermal equilibrium is reached? ?final=

Solid calcium chloride dissolves in water according to the equation below.CaCl2 (s) ➝ Ca+2 (aq) + 2 Cl – (aq)      ΔHº = –81.3 kJ/mol8.00 grams of solid CaCl2 dissolves in 45.0 grams of water initially at a temperature of 20.00 ºC in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g·ºC)]Tfinal = Answer ºC

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 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol

A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 15.2 g, and its initial temperature is −13.9 ∘C. The water resulting from the melted ice reaches the temperature of his skin, 29.9⁢ ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.   Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H 2 O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) *  Specific heat of liquid H 2 O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) *  Specific heat of gaseous H 2 O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) *

A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C.