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NGSS Chem Spring Final Review

Total questions: 48

Worksheet time: 2hrs 38mins

Name
Class
Date
1.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
2.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
3.
O2 + CS2 --> CO2 + SO2
What coefficient would go in front of the O2?
a)
1
b)
2
c)
3
d)
4
4.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
5.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
6.

Calculate ΔT\Delta T  when a substance goes from 10*C to 75*C

a)

-65*C

b)

75*C

c)

10*C

d)

65*C

7.

Calculate A 50g sample is heated with 500 joules of energy and has a 10*C temperature change. Calculate it’s specific heat.

a)

1 j/g*C

b)

250000 j/g*C

c)

500 j/g*C

d)

10 j/g*C

8.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

9.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

10.

Releasing heat into the surroundings occurs during an ___________________ reaction.

a)

Exothermic

b)

Endothermic

c)

Kinetic Energy

d)

Thermal Energy

11.

A sample of iron receives 50 J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

12.

Which law states that energy cannot be created nor destroyed, but it can be transformed or transferred?

a)

Dalton's Law

b)

law of conservation of energy

c)

Hess's Law

d)

E=mc^2

13.

What happens when kinetic energy increases?

a)

Temperature increases.

b)

Temperature decreases.

c)

Temperature is not affected by kinetic energy.

14.

A gas has ________ kinetic energy than a liquid.

a)

more

b)

less

15.

A sample of a compound has a mass of 30 g and a specific heat of 0.258 J/g*K. If its temperature drops 40 K, how much heat was released? ( q=mcΔTq=mc\Delta T  )

a)

309.6 J

b)

-309.6 J

c)

465 J

d)

-465 J

16.

When water evaporates, the process is...

a)

endothermic

b)

exothermic

17.

When wood is burned in a campfire, the process is...

a)

endothermic

b)

exothermic

18.

For an exothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

19.

For an endothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

20.

In the following reaction, A + 2B --> 3C, ΔH = 640 kJ\Delta H\ =\ 640\ kJ  . How much energy is needed to react 4 moles of A?

a)

2560 kJ

b)

1280 kJ

c)

1920 kJ

d)

3840 kJ

21.

In an exothermic reaction, heat is a...

a)

product

b)

reactant

22.

In an endothermic reaction, heat is a...

a)

product

b)

reactant

23.

The amount of heat required to raise the temperature of 1 gram of water by 1°C is known as (choose the BEST answer!)

a)

Calorie

b)

Thermodynamics

24.

According to the Law of Conservation of Energy, when energy is changed from one form to another,

a)

all matter is conserved (kept)

b)

all matter is lost (destroyed)

25.

what does c stand for?

a)

heat capacity

b)

specific heat

c)

mass

d)

temperature

26.

Mass must always be in ________ for energy calculations.

a)

kilograms

b)

grams

c)

joules

d)

calories

27.
20 g of water. specific heat of water is 4.18 J/g°C.  temperature changes from 25° C to 20° C, how much heat energy (q) moves from the water to the surroundings?
a)
400 J
b)
210 J
c)
80 J
d)
4.18 J
28.
Activation energy is required to start a chemical reaction. What is activation energy?
a)
The energy needed for a reaction to occur
b)
The minimum amount of energy needed for a reaction to potentially occur
c)
The energy added by a catalyst
d)
The energy possessed by the products
29.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
30.

A catalyst  ........... the rate of reaction by .......... the energy of activation.

a)

Decrease, increasing

b)

increase, increasing

c)

Increases, decreasing

31.

Indicate whether each of the following will: Increase / Decrease / have No effect on the rate of reaction.

 

                Decrease Particle Size              

a)

Increase

b)

Decrease

c)

No Effect

32.

Indicate whether each of the following will: Increase / Decrease / have No effect on the rate of reaction.

 

                Decrease Reactant Concentration             

a)

Increase

b)

Decrease

c)

No Effect

33.

Which energy diagram line represents the catalyzed reaction?

a)

The black line

b)

The red line

c)

It can not be determined

34.

which factor that affect reaction rate is represented?

a)

Temperature

b)

Catalyst

c)

Surface Area

d)

Concentration

35.

B represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

36.

A represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

37.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
38.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
39.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
40.

Smaller clumps allow for a _________ surface area to be exposed for the reaction.

a)
larger
b)
smaller
41.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
42.
What type a reaction is taking place in this picture?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
43.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
44.
Ions in two compounds switch. 
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
45.

Identify the reaction type:

C2H6 + O2 --> CO2 + H2O

a)

Double replacement

b)

Synthesis

c)

Acid base

d)

Combustion

46.

Identify the type of reaction:

ZnCl2 + Mg --> Zn + MgCl2

a)

Precipitate

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

47.

Identify the reaction type:

NaCl + KOH --> KCl + NaOH

a)

Double replacement

b)

Combustion

c)

Synthesis

d)

Decomposition

48.

Identify the reaction type:

H2O2 --> H2O + O2

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Acid Base

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