Quiz: Endothermic and Exothermic Rxns
By Keri Owen
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Last updated over 6 years ago
20 Questions
Note from the author:
Properties (descriptions) of endothermic and exothermic reactions.
Chemical reactions don't need energy to break apart bonds.
Chemical reactions don't need energy to break apart bonds.
In a chemical reactions new bonds form to make the products.
In a chemical reactions new bonds form to make the products.
Energy cannot be created nor destroyed.
Energy cannot be created nor destroyed.
More energy is released by products than is needed to break bonds.
More energy is released by products than is needed to break bonds.
Products have less energy than the reactants.
Products have less energy than the reactants.
It literally means "taking in heat."
It literally means "taking in heat."
Energy is needed to keep the reaction going.
Energy is needed to keep the reaction going.
Reactions feel hot to us.
Reactions feel hot to us.
An example is baking soda and vinegar.
An example is baking soda and vinegar.
Reaction feels cold.
Reaction feels cold.
Wood burning is an example.
Wood burning is an example.
Products have more energy than the reactants.
Products have more energy than the reactants.
Heat is absorbed.
Heat is absorbed.
Photosynthesis is an example.
Photosynthesis is an example.
Combustion reactions are examples.
Combustion reactions are examples.
This equation: Reactants→Products+Energy
This equation: Reactants→Products+Energy
Is the graph above respresentative of an endothermic or exothermic reaction?
Is the graph above respresentative of an endothermic or exothermic reaction?
From where does the energy for photosynthesis come?
From where does the energy for photosynthesis come?
During the photosynthesis reaction plants convert carbon dioxide and water to
During the photosynthesis reaction plants convert carbon dioxide and water to
The energy needed to start reactions is called
The energy needed to start reactions is called