Exothermic and Endothermic Processes Quiz

Do all chemical processes always release energy? Are there reactions that absorb energy?

How can we differentiate heat and temperature?

How can we measure heat?

How do we quantify the amount of heat absorbed or evolved in a reaction?

Calculate the heat change involved when 2000.0 g of water is heated from 20.0 oC to 99.7 oC in an electric kettle. The specific heat of water is 4.18 J/(g∙°C).

A student uses 225 mL of hot water in a lab procedure. Calculate the amount of heat required to raise the temperature of 225 mL of water from 20.0 oC to 100.0 oC. The specific heat of water is 4.18 J/(g∙°C). (Assume 1g=1ml)

A block of aluminum weighing 140 g is cooled from 98.4 °C to 62.2 °C with the release of 1080 joules of heat. From this data, calculate the specific heat of aluminum.

What happens when a process is exothermic?

What happens when a process is endothermic?

Will the burning of wood in a campfire be an exothermic or an endothermic process? Explain why.