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Exothermic and Endothermic Reactions

Chemistry ⇒ Chemical Reactions and Equations

Exothermic and Endothermic Reactions starts at 8 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Exothermic and Endothermic Reactions. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 11
A chemical cold pack contains ammonium nitrate and water. When activated, the pack becomes cold. What type of reaction is occurring?
A reaction has ΔH = -200 kJ. Is this reaction exothermic or endothermic?
A student mixes barium hydroxide and ammonium chloride in a beaker. The beaker becomes very cold. What type of reaction is this?
Calculate the enthalpy change (ΔH) for a reaction if the energy absorbed is 150 kJ and the energy released is 100 kJ.
Describe how you would experimentally determine if a reaction is exothermic or endothermic.
Describe what happens to the temperature of the surroundings during an endothermic reaction.
Explain the difference between exothermic and endothermic reactions in terms of energy transfer.
Explain why combustion reactions are always exothermic.
Explain why the dissolution of some salts in water is endothermic while for others it is exothermic.
Is the process of dissolving sodium hydroxide in water exothermic or endothermic?
Is the process of rusting of iron exothermic or endothermic?
A chemical reaction has a positive enthalpy change (ΔH > 0) and leads to a decrease in temperature of the surroundings. What type of reaction is this?
A student dissolves calcium chloride (CaCl2) in water and observes a significant increase in temperature. Explain, in terms of enthalpy change and energy flow, why this occurs.
Consider the following reaction: N2(g) + 3H2(g) → 2NH3(g) + 92 kJ Is this reaction exothermic or endothermic? Justify your answer based on the information provided.
Explain, with reference to bond energies, why some reactions are endothermic while others are exothermic.
The decomposition of calcium carbonate is represented by the equation: CaCO3(s) → CaO(s) + CO2(g); ΔH = +178 kJ/mol Calculate the total energy absorbed when 10.0 g of CaCO3 decomposes. (Molar mass of CaCO3 = 100 g/mol)