an 33.777g piece of metal is heated in a hot water bath at 98.5°C and then cransferred to a coffee-cup calorimeter containing 50.0mL of water. The initial water temperature was 22.9°C and the final water temperature was 27.3°C. Determine the specific heat of the metal (Cmetal). Ccal = 21.0J/°C & Cwater = 4.184 J/g*°C. %3D Report your answer to 3 sf and in J/g*°C. Your Answer:

A piece of lead (mass = 2.85 g) at 10.3 C is placed in a Styrofoam coffee cup containing 7.55 mL of water at 52.3 C. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature should be? The specific heat capacity of lead = 0.128 J/g°C and water = 4.18 J/g°C. density of water = 1.00 g/mL

The temperature of the solution increases from 21.3 °C to 38.2 °C. 0.468 g Mg reacting0.0193 mol Mg reacting80.844 g HCl solution The energy released is given by q = specific heat × mass × temperature changeThe solution is almost all water, so we use the specific heat capacity of water, 4.18 J/g•°C. What is the quantity of heat released? Enter your answer as a positive value.

When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy change for this process is called the enthalpy of solution. To measure it, 175.0 g of water was placed in a coffee-cup calorimeter and chilled to 10.0 °C. Then 49.0 g of pure sulfuric acid, also at 10.0 °C, was added, and the mixture was quickly stirred with a thermometer. The temperature rose rapidly to 14.9 °C. Assume that the specific heat capacity of the resulting sulfuric acid solution is 4.19 J/g °C. Calculate the quantity of thermal energy transferred, Q, for the formation of this solution, and calculate the molar enthalpy of solution in kilojoules per mole of H₂SO4.