Interpreting Rates Graphs Flashcards

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On a graph of a reaction, what quantity is usually shown on the x-axis?

Time from the start of the reaction.

On a rate of reaction graph, what is usually shown on the y-axis?

The amount of reactant used up or product made, such as mass in grams or volume of gas in cm³.

What does the steepness (gradient) of a reaction graph tell you?

It tells you how fast the reaction is going: a steeper line means a faster rate of reaction.

How can you tell from a rate graph that a reaction has finished?

The line becomes horizontal (flat), showing that the amount no longer changes with time.

How do you work out the average rate of reaction from a graph between two times?

Find the change in amount from the graph and divide it by the change in time: rate = change in amount ÷ time taken.

What is meant by the initial rate of a reaction on a graph?

It is the rate right at the start of the reaction, shown by the gradient of the line near time = 0.

Two graphs of volume of gas against time reach the same final volume. One line is steeper at the start. What does this show?

Both reactions make the same amount of gas, but the one with the steeper line is faster.

If a reaction graph is curved and becomes less steep over time, what does this tell you about the rate?

The reaction is slowing down because the rate is getting lower as the reactants are used up.

What units would you use for the rate of reaction if volume is measured in cm³ and time in seconds?

cm³ per second (cm³/s).

On a graph of mass of a flask against time, the mass goes down then levels off. What is happening in the reaction?

A gas is being given off, so the mass falls at first; when the line levels off, the reaction has finished.

How can you find the rate of reaction at a single point on a curved graph?

Draw a tangent (a straight line just touching the curve) at that point and find its gradient.

How does a higher temperature or a catalyst show on a graph of volume of gas against time?

The line is steeper and levels off sooner, showing a faster reaction, but it often reaches the same final volume.

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