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GCSE Chemistry Unit 2 > Rates of reaction > Flashcards

Flashcards in Rates of reaction Deck (7)
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1

The equation for the reaction is:
sodium thiosulfate + hydrochloric acid → sodium chloride + water + sulfur dioxide + sulfur
Explain why the solution goes cloudy. [2]

- sulfur forms...
- ...which is solid / a precipitate

2

State the effect that increasing the temperature of the sodium thiosulfate solution has on the rate of the reaction.
Explain this effect in terms of particles and collisions. [4]

- rate increases...
- ...because particles move faster...
- ...so particles are more likely to collide
- more particles have energy greater than the activation energy

3

Explain, in terms of particles and collisions, the effect that increasing the surface area has on the rate of reaction. [2]

- the rate increases...
- ...because of more frequent collisions between particles

4

Give one reason why using a catalyst reduces costs. [1]

- it increases the rate of reaction
- it reduces the energy required
- lower temperatures can be used
- catalysts don't get used up

5

Suggest one improvement the student could make to the apparatus when investigating the temperature change. [2]

- add a lid...
- ...to reduce / stop heat loss
- use a digital thermometer...
- ...for more accurate data

6

State the effect of increasing the pressure on the rate of reaction.
Explain your answer in terms of particles. [3]

- rate increases...
- ...because particles are closer together...
- .., so particles are more likely to collide

7

What is meant by the activation energy? [1]

the (minimum) amount of energy (particles must have) to react