Exothermic and Endothermic Processes Quiz

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

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How can we differentiate heat and temperature?

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How can we measure heat?

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

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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).

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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)

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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.

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What happens when a process is exothermic?

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What happens when a process is endothermic?

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

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