A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1 °C. At equilibrium the temperature of the water and metal was 33.5 °C. What was ΔT for the water? What was ΔT for the metal? Using the specific heat of water (4.184 J/g °C), calculate how much heat flowed into the water calculate the specific heat of the metal. What is the average specific heat capacity of the unknown metal in this experiment? What is the unknown metal?

2. Calculate the amount of heat required to raise the temperature of 950.0 mL of a solution from 22.5 °C to 38.0 °C if the solution has a density of 1.04 g mL-l and a heat capacity of 4.08 J K-l g. 3. This reaction: CH4(g) + 202(g) → CO2(g) + 2H2O(1) produces 56.0 kJ of heat when 1.00 g of methane is burned. What is the molar heat of combustion for CH4? 4. In thermodynamics heat is represented by the letter 'q' and q is negative for processes which lose heat to the surroundings (i.e. exothermic processes). What is q for burning one mole of methane? 5. What mass of methane would need to be burned in order to generate the heat required to raise the temperature of the solution in question 2? (Hint: look at question 3 for some relevant data) 6. In this lab class you will measure the enthalpy change for hydrochloric acid reacting with sodium hydroxide. What effect, if any, would using nitric acid instead of hydrochloric acid have on the enthalpy changes measured in this experiment? Why?…

When 200.0 mL of 0.862 M HCI is mixed with 200.0 mL of 0.431 M Ba(OH)2 in a coffee cup calorimeter, the temperature of the solution increases from 21.35°C to 27.05°C. Given the specific heat of solution of 4.18 J g1 °C-l and assuming the density of each solution to be 1.00 g/mL, what is the heat of reaction in kJ per mole of HCl? The neutralization reaction is: 2 HCI(aq) + Ba(0H)2(aq) → BaCl2(aq) + 2 H20(1) Select one: -55.3 kJ/mol HCI -9.53 kJ/mol HCI O - 110.6 kJ/mol HCI O 110.6 kJ/mol HCl 55.3 kJ/mol HCI O 9.53 kJ/mol HCI ВАCK Question 5 of 6 NEXT étv A

100.0 mL of 1.00 M HBr at 22.5 °C is combined with 100.0 mL of 1.00 M LiOH at 22.5 °C. The mixture reaches a temperature of 29.2 °C. Assume the density of the solutions is 1.00 g/mL and their specific heat capacity is the same as pure water. What is the molar heat of reaction?