When iron metal is mixed with hydrochloric acid, the following reaction occurs: 2Fe(s) + 6HCl(aq) → 2FeCl3(aq) + 3H2(g). When 1.104 g of iron is mixed with 26.023 g of HCl in a coffee cup calorimeter, the temperature rises from 25.2 °C to a final temperature. What type of reaction is this?

When 1.045 g of Na2O is added to 50.0 mL of water at 25.0 °C in a calorimeter, the temperature of the water increases to 54.4 °C. Assuming that the specific heat of the solution is 4.18 J/(g·°C) and that the calorimeter itself absorbs a negligible amount of heat, calculate the heat absorbed by the solution.

When 12.2 g of an ionic compound (molar mass = 86.49 g/mol) is dissolved in 133 g of water in a coffee-cup calorimeter, the temperature changes from 21.24 °C to 16.34 °C. Calculate ΔHsolution for this ionic compound in kJ/mol. Use c = 4.18 J/(g°C) for water.

When 4.00 g of Ba(s) is added to 50.00 g of water in a container open to the atmosphere, the reaction shown below occurs, and the temperature of the resulting solution rises from 22.00°C to 77.62°C. If the specific heat of the solution is 4.18 J/(g°C), what is the nature of the reaction?

When 5.03 g of solid potassium hydroxide (KOH) are dissolved in enough distilled water to give 100 mL of solution in a coffee-cup calorimeter, the temperature of the liquid increases from 23.0°C to 34.7°C. Based on this observation, is the dissolution of KOH in water an endothermic or exothermic reaction?

When iron metal is mixed with hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2°C to a final temperature. What type of reaction is occurring?

Which statement is FALSE regarding endothermic and exothermic reactions?

Which statement is true regarding the energies involved in an endothermic reaction?

What is the energy lost when 11.3 g of gold cools from 224 °C to 117 °C, given that the specific heat capacity of gold is 0.129 J/g°C?