I place a cube of steel 100 cm³ in a room and place a 100 cm³ cube of oak next to it. The room they are in is 37⁰C. They sit there for 1 day. If I measure their temperature the next day with a probe, what will their respective temperatures be? (assume that what they are sitting on is not affecting their temperature)

They are unchanged from the original Temperature

Calorimetry and Thermochemistry

Quiz

•

Chemistry

•

10th Grade - University

•

Practice Problem

•

Hard

•

NGSS

HS-PS3-4, HS-PS1-4, HS-PS3-2

+3

Standards-aligned

Charles Martinez

FREE Resource

21 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The unit(s) for heat are?

calories

joules

calories or joules

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

135 g of aluminum (initially at 400^oC) are mixed with an unknown mass of water (initially at 25^oC). When thermal equilibrium is reached, the system has a temperature of 80^oC. Find the mass of the water.

197.2g

168.6g

168.6J

23.1g

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

3.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

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?

2.56 J/g°C

0.391 J/g°C

5.29 J/g°C

3.50 J/g°C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-2

NGSS.HS-PS3-4

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

In the lab, an experimenter mixes 75.0 g of water (initially at 30^oC) with 83.8 g of a solid metal (initially at 600^oC). At thermal equilibrium, he measures a final temperature of 50.0^oC. What was the specific heat of the metal?

0.672 J/g ⁰C

0.533 ⁰C

1.156 J/g ⁰C

0.133 J/g ⁰C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

5.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

The specific heat of a substance is the amount of energy needed to raise the temperature of one gram, one degree Celsius of a substance.

True

False

sometimes

Tags

NGSS.HS-PS3-4

6.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

As a reaction is taking place, the student notices that the temperature has dropped. This indicates that the system has increased in energy. What type of process is this?

Endothermic

Exothermic

Tags

NGSS.HS-PS1-4

7.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

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

g /J C

J/g⁰C

kJ/g

KJ/⁰Cg

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Calorimetry and Thermochemistry

21 questions

The unit(s) for heat are?

135 g of aluminum (initially at 400^oC) are mixed with an unknown mass of water (initially at 25^oC). When thermal equilibrium is reached, the system has a temperature of 80^oC. Find the mass of the water.

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?

In the lab, an experimenter mixes 75.0 g of water (initially at 30^oC) with 83.8 g of a solid metal (initially at 600^oC). At thermal equilibrium, he measures a final temperature of 50.0^oC. What was the specific heat of the metal?

The specific heat of a substance is the amount of energy needed to raise the temperature of one gram, one degree Celsius of a substance.

As a reaction is taking place, the student notices that the temperature has dropped. This indicates that the system has increased in energy. What type of process is this?

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

Using the heat equation, what would the formula look like if we were solving for change in temperature?

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 .10 J/g°C, what is the mass of the iron sample?

What would be the effect on particles if more heat is supplied to the system?

Access all questions and much more by creating a free account

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Calorimetry and Thermochemistry

21 questions

The unit(s) for heat are?

135 g of aluminum (initially at 400oC) are mixed with an unknown mass of water (initially at 25oC). When thermal equilibrium is reached, the system has a temperature of 80oC. Find the mass of the water.

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?

In the lab, an experimenter mixes 75.0 g of water (initially at 30oC) with 83.8 g of a solid metal (initially at 600oC). At thermal equilibrium, he measures a final temperature of 50.0oC. What was the specific heat of the metal?

The specific heat of a substance is the amount of energy needed to raise the temperature of one gram, one degree Celsius of a substance.

As a reaction is taking place, the student notices that the temperature has dropped. This indicates that the system has increased in energy. What type of process is this?

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

Using the heat equation, what would the formula look like if we were solving for change in temperature?

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 .10 J/g°C, what is the mass of the iron sample?

What would be the effect on particles if more heat is supplied to the system?

Access all questions and much more by creating a free account

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

135 g of aluminum (initially at 400^oC) are mixed with an unknown mass of water (initially at 25^oC). When thermal equilibrium is reached, the system has a temperature of 80^oC. Find the mass of the water.

In the lab, an experimenter mixes 75.0 g of water (initially at 30^oC) with 83.8 g of a solid metal (initially at 600^oC). At thermal equilibrium, he measures a final temperature of 50.0^oC. What was the specific heat of the metal?

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