Rates Of Reaction: An Intro Flashcards

1
Q

Define the term rate of reaction

A

Rate of reaction is a measure of how quickly a reactant is used up, or a product is formed. So in simpler terms, how fast the reactant are changed into products

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2
Q

Give two examples of what a slow reaction would be

A

– rusting of metal (one of the slowest is rusting of specifically iron)
– chemical weathering (like the effects of acid rain on limestone buildings)

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3
Q

List an example of a moderately paced reaction

A

A metal (specifically magnesium here) reacting with an acid (to produce a gentle stream of bubbles)

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4
Q

List an example of a faster paced reaction

A

Burning. And explosions. They happen in a split second- in fact less than a second and they produce a lot of gas

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5
Q

How can you calculate the speed of a reaction?

A

Recording the amount of product formed or the amount of reactant used over the time of the reaction

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6
Q

Say you plot a graph of the reaction. What does a steep line mean? And what happens when it grows flat?

A

The steeper the line, the faster the rate of the reaction, however, the line will gradually get flatter as the reactants get used up.

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7
Q

What do quicker reactions look like on a graph?

A

Quicker reactions have a steeper line and reach the flat point at the least amount of time.

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