3.1.6 Chemical equilibria

Question 1

Explain collision theory

Answer 1

1) particles must collide to react
2) chemical bonds must be broken when particles react
3) particles must collide in the correct orientation

Question 2

How can the rate of reaction be increased?

Answer 2

• increased concentration of reactants
• increase gas pressure

Question 3

What is the transition state?

Answer 3

the point where existing chemical bonds are in the process of breaking and new ones are in the process of forming

Question 4

define activation energy

Answer 4

enthalpy change between reactants and the highest point on the curve (transition state)

Question 5

What does the highest point on the curve represent?

Answer 5

formation of the transition state

Question 6

What do catalysts do?

Answer 6

allow a reaction to take place via an alternative pathway with lower activation energy than the uncatalysed reaction

Question 7

Benefits of using a catalyst

Answer 7

-reactions could be done at lower energy so ECONOMIC benefit
less fossil fuels burned to produce energy means an ENVIRONMENTAL benefit

Question 8

Define heterogenous catalysts

Answer 8

different pysical state (phase) to reactants

Question 9

Define homogeneous catalysts

Answer 9

catalyst in the same physical state as the reactants

Question 10

https://youtu.be/RHT7SocYKZk?list=PL9IouNCPbCxV32VF190X1WTIBxMkTpJSt&t=72