Honors Unit 4 Quiz

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

• 25g

• 30g

• 20g

• 50g

What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)

• 0.111 J/g°C
• 1.29 J/g°C
• 0.129 J/g°C
• 22225.85 J

Calorimetry Question:
A piece of metal with a mass of 32.8 g is heated to 100.5°C and dropped into 138.2 g of water at 20.0°C.  The final temperature of the system is 30.2°C.  What is the specific heat capacity of the metal? (show your work)

• 2.56 J/g°C
• 0.391 J/g°C
• 5.29 J/g°C
• 3.50 J/g°C

Between which points is the temperature of the substance remaining constant?

• A-B only

• A-B, C-D, and E-F

• B-C only

• B-C and D-E

The melting point of the sample is

• -60 ºC

• 20 ºC

• 60 ºC

• 100 ºC

What scenario fits the highlighted areas?

• ice at -20⁰C to water at 75⁰C

• ice at 0⁰C to water at 75⁰C

• ice at 0⁰C to water at 100⁰C

• water at 0⁰C to water at 75⁰C

A 32.0 gram sample of water at 20.0⁰C is heated until it is steam at 232⁰C.

How much heat energy (in joules) was added?

• 100,700 J

• 72,300 J

• 28,400 J

• 7,770 J

• 90,800

How many Joules of energy are required to make 50.0 grams of ice at 0 ^οC completely melt?

• 334 J

• 0 J

• 33,400 J

• 16,700 J

Calculate the energy needed to completely boil away 30 g of water at 100 ⁰C .

• 67,800 J

• 2260 J

• 226,000 J

• 100 J

Given the thermochemical equation, calculate the heat evolved when 74.6 g of sulfur dioxide (molar mass = 64.07 g/mol) is converted to sulfur dioxide.

• -115 kJ

• 115 kJ

• -115.39 kJ

• 115.39 kJ