Free Printable Thermodynamics Review District test

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Thermodynamics Review District test

Total questions: 30

Worksheet time: 3hrs 30mins

Name

Class

Date

ΔH value in an endothermic reaction is a positive number.

True

False

_?_ is the amount of energy required to raise the temperature of 1 gram of any substance 1^oC.

Specific heat

A calorie

Thermal energy

Conduction

As 120 g of hot milk cools in a mug, it transfers 20, 000 J of heat to the environment. What is the temperature change of the milk? The specific heat of milk is 2.6 J/g·°C. (Q=mcΔT)

64 °C

1.56 °C

640 °C

cannot be determined

If 100 g of aluminum at 145ºC gains 6,800 J of heat, what is the final temperature (T_final) of the aluminum? Aluminum has a specific heat of 0.897 J/gºC. (Q=mcΔT)

-69°C

0.52°C

221°C

The Q of water is 100. If he ΔT=20⁰C and the change in mass of the biscuit, Δm =1.35g.Find the enthalpy of the biscuit in kJ/g. (Q=mcΔT)

6.19

61.9

6193

3.703

The Q of water is 200. If he ΔT=45.6⁰C and the change in mass of the biscuit, Δm =5.35g.Find the enthalpy of the biscuit in kJ/g. (Q=mcΔT)

7126

0.8189

7.13

38.12

How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0^oC to 50.0^oC? the specific heat of aluminum is 0.900J/g^oC

450

-450

225

-225

How do you calculate Enthalpy of a reaction?

ΔH = ΔH_products- ΔH_reactants

ΔT = q / mC

ΔG = ΔH -TΔS

E = mc²

Which statement is true regarding endothermic reactions?

a) Temperature change is positive and enthalpy change is positive

b) Temperature change is positive and enthalpy change is negative

c) Temperature change is negative and enthalpy change is positive

d) Temperature change is negative and enthalpy change is negative

10.

Endothermic reactions feel

warm

cold

11.

Define 'Enthalpy'

a) Energy stored in the movement of molecules in a substance

b) The opposite of temperature

c) The temperature of a molecule

d) Energy stored in the chemical bonds in a substance (Heat)

12.

If the entalpy of reaction is $-\Delta H$

Exothermic

Endothermic

I don't know

13.

What do we call the relationship between thermal energy, heat and work?

Closed System

Entropy

Conductors

Thermodynamics

14.

For the formula:
Q= m c ∆T
The units for specific heat are:

g /J C

°C/g J

kJ/g

J/g°C

15.

Thermal energy ALWAYS moves from _____ to _____.

solid to liquid

ice to water

hot to cold

solid to gas

16.

If the specific heat of water is 4,186 J/kg∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C?

-80,371.2

44,938.6

80,371.2

112,575.9

17.

3g of water are at temperature 5 C. The water reaches the boiling point 100 C. The
specific heat capacity of water = 4.180 J/g C

2547.5 J

1191.3 J

1191.3 g

11.193 kg

18.

The specific heat of aluminum is 0.21 J/g°C. How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?

105 J

10.5 J

1.05 J

19.

20 g of water. specific heat of water is 4.18 J/x°C. temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?

-418 Joules

209 J

83 J

4.18 J

20.

What is happening to the average kinetic energy of the particles during segment B C?

Increasing

Stays the same

Decreasing

Not represented on the diagram

21.

What is the equation to determine the heat required to change the temperature from 0 °C to 15 °C?

Q = mC $\Delta T$

Q = mHf

Q = mHv

C = Q/m $\Delta T$

22.

How many Joules of heat energy are needed to raise the temperature of 10.0 g of aluminum from 22 °C to 55 °C, if the specific heat of aluminum is 0.90 J/g°C? What is the unknown in this problem?

$\Delta T$

23.

In an exothermic reaction …….

more heat energy is released than absorbed

more heat energy is taken in than released

nothing happens

energy transfer stops when temperature increases

24.

Rate your confidence on this subject.

I got this!

I am okay but need more practice.

I am confused

25.

What type of system is this?

Open

Closed

Isolated

26.

What type of system is this?

Open

Closed

Isolated

27.

What type of system is this?

Open

Closed

Isolated

28.

What type of system is this?

Open

Closed

Isolated

29.

The exchange of mass and energy is what type of system?

Open

Closed

Isolated

30.

The exchange of energy but not mass is what type of system?

Open

Closed

Isolated

Reset

Thermodynamics Review District test

Total questions: 30

Worksheet time: 3hrs 30mins

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