Benchmark 4 review day 1 (Unit 10 thermo,K&E)

Wednesday 5/11- Benchmark review- Unit 10

Announcements/Reminders

Agenda:

​

• 12 class DAYS until final!

• Thurs 5/9- English EOC, 1st &2nd block

• Mon 5/13-Benchmark #4

• 5/22- no school- Biology EOC

• 5/23- USH EOC

• 5/28- final exam (1st&2nd periods)

• ​Unit 10 review

Bellwork: ​​

Multiple Choice

Can energy be created?

• Yes

• No

Multiple Choice

Which of the following is not a form of energy?

• Thermal (heat)

• temperature

• Nuclear
• Mechanical
• light

Multiple Choice

Heat flows from _______ to ______ objects

• cooler to warmer

• warmer to warmer

• warmer to cooler

• cooler to cooler

Multiple Choice

Phase changes: ice to water to steam

• endothermic

• exothermic

Multiple Choice

Phase changes: steam to water to ice

• endothermic

• exothermic

Multiple Select

Select all the processes that are exothermic. The system is underlined in each example.

• Your hand gets cold when you touch ice.

• The ice gets warmer when you touch it.

• Water boils in a kettle being heated on a stove.

• Water vapor condenses on a cold pipe.

• Ice cream melts.

Multiple Select

Select all the processes that are endothermic. The system is underlined in each example.

• Your hand gets cold when you touch ice.

• The ice gets warmer when you touch it.

• Water boils in a kettle being heated on a stove.

• Water vapor condenses on a cold pipe.

• Ice cream melts.

Multiple Choice

If they energy required to break the bonds is greater than the energy given out by making new bonds the reaction is

• Exothermic
• Endothermic
• Neutralisation

Multiple Choice

$$O_2\left(g\right)\ +\ 2\ H_2\ \left(g\right)\ \rightarrow\ 2\ H_2O\ \left(g\right)\ +\ Energy$$  

• endothermic

• exothermic

Multiple Choice

ΔH value in an endothermic reaction is a positive number.

• True
• False

Multiple Choice

A catalyst works by

• changing the order of the reaction
• increasing the temperature
• lowering the activation energy
• making the activated complex

Multiple Choice

What is the Heat of Reaction $$\Delta H$$  for this reaction?

• -200 KJ

• 200 KJ

• 400 KJ

• -300 KJ

Multiple Choice

How much activation energy is needed for this reaction?

• 300 KJ

• 500 KJ

• 400 KJ

• 100 KJ

Multiple Choice

What type of reaction is this?

• Exothermic

• Endothermic

• Energy Producing

• No way to tell

Multiple Choice

What kind of reaction is this: 2KI + MgCl₂ + 200KJ ----> 2KCl + MgI₂

• Endothermic

• Exothermic

Multiple Choice

What letter represents the energy of the products?

• A
• B
• C
• D

Multiple Choice

What letter represents the activation energy?

• A
• B
• C
• D

Multiple Choice

What letter represents ΔH?

• A
• B
• C
• D

Multiple Choice

Which letter represents the activation energy?

• B
• E
• C
• D

Multiple Choice

What is the PE of the reactants?

• 100 kJ
• 175 kJ
• 50 kJ
• 75 kJ

​nIonic solutions have faster reactions than molecule compounds. (bonding)

néTemp. é Rate

né conc. érate

né surface area é rate

né Pressure é rate, ê P ê rate 

nCatalysts speed up reactions.

​Quick review- Factors affecting rate

Multiple Choice

This symbol indicates that a reaction is _____

• reversible

• irreversible

​→

Multiple Choice

When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in

• Chemical Equilibrium
• Chemical Balance
• Chemical Constant
• Chemical Reaction

Multiple Choice

Which of the following is NOT true at equilibrium?

• The forward and reverse reactions proceed at the same rate.
• The concentrations of reactants and products do not change.
• The concentration of the reactants is equal to the concentration of the products.
• The forward and reverse reactions continue to occur.

​Concentration increase shift away from increase

• Concentration decrease shift toward decrease

• 🡹 pressure shifts in direction of fewer gas molecules.

• 🡻 pressure shifts in direction of more gas molecules

• 🡹 temperature favors endothermic reaction

  • Shift away from heat

• 🡻 temperature favors exothermic reaction

  • Shift towards heat

​Equilibrium shifts due to stresses:

​Example- The Haber process (making ammonia NH₃)

​N2 (g) + 3 H2 (g) ⮀ 2 NH3 (g) + heat

1. 🡹 [N2]

2. 🡻 [H2]

3. 🡹 [NH3]

4. 🡻 [NH3]

5. 🡹 pressure

6. 🡻 pressure

7. 🡹 temperature

8. 🡻 temperature

Multiple Choice

Le Chaltelier's Principle states that if a chemical system at equilibrium is stressed,

• the system will adjust to increase the stress
• the system will adjust to reduce the stress
• the system will not adjust

Multiple Choice

(🡹 pressure shifts in direction of fewer gas molecules)

(🡻 pressure shifts in direction of more gas molecules )

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat

Increasing the pressure will cause the equilibrium to:

• Shift right

• Shift left

• Have no change

• Speed up

Multiple Choice

🡹 temperature favors endothermic reaction Shift away from heat 🡻 temperature favors exothermic reaction Shift towards heat

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat

Increasing the temperature will cause the equilibrium to:

• Shift right

• Shift left

• Have no change

• Speed up

Multiple Choice

(Concentration increase shift away from increase)

(Concentration decrease shift toward decrease)

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat

Decreasing H₂ will cause the equilibrium to:

• Shift right

• Shift left

• Have no change

• Speed up

Multiple Choice

(Concentration increase shift away from increase)

(Concentration decrease shift toward decrease)

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat

Removing N₂ will cause the equilibrium to:

• Shift right

• Shift left

• Have no change

• Speed up

Multiple Choice

(Concentration increase shift away from increase)

(Concentration decrease shift toward decrease)

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat

Increasing H₂ will cause the equilibrium to:

• Shift right

• Shift left

• Have no change

• Speed up

Multiple Choice

For the reaction...
SO_2(g) + O_2(g) <−>  SO_3(g)
If the concentration of SO_2(g)  is increased, the equilibrium of the reaction will ___________.

• shift to the left
• shift to the right
• not shift