7. For the following scenarios what is the metal? a. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. platinum niobium vandium titanium C (kJ/kg K) 0.13 0.27 0.39 0.54 b. A 25.6 g piece of metal was taken from a beaker of boiling water at 100.0 °C and placed directly into a calorimeter holding 100.0 mL of water at 25.0 °C. The calorimeter heat capacity is 1.23 J/K. Given that the final temperature at thermal equilibrium is 26.2 °C, determine the specific heat capacity of the metal.

Consider the reaction.   2Fe2O3⟶4Fe+3O2.    Δ?∘rxn=+824.2 kJ   The formation of 12.0 g of O2 results in the release or absorption of what amount of heat? in kJ

When a 4.00 g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity of 1.47 kJ · K-, the temperature decreases by 0.360 K. Calculate the molar heat of solution of RbBr. AH soln -2 1.28 x10 kJ/mol Incorrect

An experiment was performed to calculate the heat of solution for potassium fluoride. Use the following data to determine its heat of solution. Assume that the specific heat capacity of the solution produced is the same as that of water, 4.184 J⁄g·°C. Identity of Salt   KF Mass of water in calorimeter (g)   52.42 Mass of salt sample (g)   7.32 Initial temperature of Calorimeter (°C)   20.8 Final temperature of Calorimeter (°C)   30.3 Report your answer in kJ/mol to 3 significant figures.

The specific heat capacity of silver is 0.24 J/°C.g. a. Calculate the energy required to raise the temperature of 143.0 g Ag from 268 K to 292 K. Energy = b. Calculate the energy required to raise the temperature of 1.0 mole of Ag by 1.0°C (called the molar heat capacity of silver). Molar Heat Capacity= J/°C-mol c. It takes 1.18 kJ of energy to heat a sample of pure silver from 12.4°C to 15.4°C. Calculate the mass of the sample of silver. g Mass=

A candy bar has a total mass of 75.0 grams. In a calorimetry experiment, a 1.25-g sample of this candy bar was burned in a calorimeter surrounded by 1000 g of water. The temperature of the water in contact with the burning candy bar was measured and found to increase from an initial temperature of 21.2°C to a final temperature of 24.3°C. a. Calculate the amount of heat in calories released when the 1.25-g sample burned. (show the work you did)

40.0 g of an unknown metal at 100.0°C is added to 50.0 g of water at 30.0°C. When the system reaches equilibrium, the temperature is 34.5°C. What is the specific heat of the metal?

12. In an experiment, 5.260 g of potassium hydroxide is mixed with a dilute solution of hydrochloric acid. A neutralization reaction occurs. The hydrochloric acid is in excess. The specific heat capacity for water is 4.184 J/g. °C. The following data are obtained: Initial temperature of HCl Volume of HCl Final temperature of solution after mixing Calculate the molar enthalpy of reaction (AH₂) for potassium hydroxide. 24.5 °C 200.0 mL 31.4 °C

Simple Calorimetry. A piece of solid aluminum at 15.0°C is immersed in 12.3 g of nitrogen gas which is initially at 51.1°C and the system is allowed to equilibrate. Given that the specific heat of solid aluminum is 0.908 J/K/g and the specific heat of nitrogen gas is 1.0 J/K/g, what is the mass of the piece of solid aluminum if the final temperature is 34.7°C?

10. Can you show me how to solve this problem