rates of reaction Flashcards

1
Q

Practical: Investigating surface area Affecting Rate of Reaction

A

Put large marble chips in acid → measure gas produced every 30 seconds.

Repeat with crushed marble chips (smaller pieces = bigger surface area).

Compare how fast the gas is produced.

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2
Q

Practical: Investigating concentration Affecting Rate of Reaction

A

Keep the mass of marble chips the same.

Use different concentrations of acid.

Measure volume of gas produced over time.

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3
Q

Practical: Investigating temperature Affecting Rate of Reaction

A

Put sodium thiosulfate solution in a flask.

Heat it to a certain temperature (use a water bath).

Add HCl and start a timer.

Time how long it takes for a black “X” under the flask to disappear.

Repeat at different temperatures (e.g., 20°C, 40°C, 60°C).

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4
Q

Practical: Investigating use of a catalyst Affecting Rate of Reaction

A

Add hydrogen peroxide into a flask.

Add a small amount of MnO₂ powder.

Measure the volume of oxygen produced over time.

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4
Q

how does surface area affect ROR

A

Breaking a solid into smaller pieces increases its surface area.

More particles are exposed and available to react.

This leads to more frequent collisions between reactant particles.

✅ Result: Rate of reaction increases.

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5
Q

how does increasing gas pressure affect ROR

A

Increasing pressure means gas particles are squeezed closer together.

This increases the frequency of collisions between particles.

✅ Result: Rate of reaction increases.

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5
Q

how does increasing temperature affect ROR

A

Increasing temperature gives particles more energy.

Particles move faster → collide more often and with more energy.

More collisions have enough energy to overcome the activation energy.

✅ Result: Rate of reaction increases.

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5
Q

how does concentration increase affect ROR

A

Increasing concentration means more reactant particles in the same volume.

Particles are closer together, so collisions happen more frequently.

✅ Result: Rate of reaction increases.

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5
Q

how does a catalyst affect ROR

A

A catalyst lowers the activation energy needed for a reaction.

This means more collisions are successful (more particles have enough energy).

✅ Result: Rate of reaction increases.

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6
Q

what is a catalyst

A

s a substance that increases the rate of a reaction, but is
chemically unchanged at the end of the reaction

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7
Q

how does a catalyst work

A

by providing an alternative pathway with lower activation
energy

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8
Q

What do you measure in the practical investigating surface area and concentration?

A

Measure the volume of gas produced (e.g., CO₂) or time taken for a set volume of gas to be produced.

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9
Q

steps for Effect of Surface Area of Marble Chips

A

Set up the equipment (flask, acid, marble chips, gas syringe).

Step 1: Change surface area of marble chips (use small pieces or powder, and larger chunks for comparison).

Step 2: Change concentration of hydrochloric acid (e.g., 0.5 M, 1.0 M, 2.0 M).

Step 3: Start the reaction and measure the volume of CO₂ produced at regular intervals (e.g., every 30 seconds).

Step 4: Record the time taken for a fixed volume of gas (e.g., 50 cm³) to be produced.

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10
Q

What do you measure in the practical investigating catalysts on hydrogen peroxide?

A

Measure the volume of oxygen gas produced when hydrogen peroxide decomposes with a catalyst.

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11
Q

steps for effect of concentration of Hydrochloric Acid on the Rate of Reaction

A

Set up the equipment (flask, hydrogen peroxide, catalyst, gas syringe).

Step 1: Add a fixed volume of hydrogen peroxide (e.g., 50 cm³).

Step 2: Add a fixed mass of the solid catalyst (e.g., MnO₂, CuO, or KI).

Step 3: Start the reaction and measure the volume of oxygen gas produced at regular intervals (e.g., every 30 seconds).

Step 4: Repeat with different catalysts.

Step 5: Compare the volume of oxygen gas produced for each catalyst.

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