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 0.418 g of pentene, C5H12, is burned in a bomb calorimeter, the temperature rises by 4.21 °C. The heat capacity of the calorimeter is 2.46 kJ/°C. Calculate the combustion energy (ΔE) for pentene, C5H12, in kJ/g.

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 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 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?