Specific Heat Equation

Presentation

•

Chemistry

•

9th - 12th Grade

•

Practice Problem

•

Hard

Jeffrey Oates

Used 2+ times

FREE Resource

6 Slides • 30 Questions

Multiple Choice

Identify the variable for the following unit:

grams

Multiple Choice

Identify the variable for the following unit:

joules per gram per degree Celsius

Multiple Choice

Identify the variable for the following unit:

Celsius

Multiple Choice

Identify the variable for the following unit:

joules

Multiple Choice

What variable is the number 700.?

How much energy is needed to increase the temperature of 700. g of water from 22°C to 98°C? The specific heat of water is 4.18 J/g°C.

Multiple Choice

What variable is the number 4.18?

How much energy is needed to increase the temperature of 700. g of water from 22°C to 98°C? The specific heat of water is 4.18 J/g°C.

Multiple Choice

What is the change in temperature?

ΔT = T_final - T_inital

How much energy is needed to increase the temperature of 700. g of water from 22°C to 98°C? The specific heat of water is 4.18 J/g°C.

-76°C

76°C

120°C

88°C

Multiple Choice

What variable is the goal?

How much energy is needed to increase the temperature of 700. g of water from 22°C to 98°C? The specific heat of water is 4.18 J/g°C.

Multiple Choice

Select the derived equation to solve for the goal?

How much energy is needed to increase the temperature of 700. g of water from 22°C to 98°C? The specific heat of water is 4.18 J/g°C.

$Q=mc\Delta T$

$\Delta T=\frac{Q}{mc}$

$m=\frac{Q}{c\Delta T}$

$c=\frac{Q}{m\Delta T}$

Multiple Choice

Solve:

How much energy is needed to increase the temperature of 700. g of water from 22°C to 98°C? The specific heat of water is 4.18 J/g°C.

2 220 000 J

2 220 J

22 200 J

222 000 J

Multiple Choice

What variable is the number 1240?

An unknown mass of silver is heated with 1240 J of energy and increases in temperature by 50°C, what is the mass of the silver? The specific heat of silver is 0.24 J/g°C

Multiple Choice

What variable is the number 0.24?

An unknown mass of silver is heated with 1240 J of energy and increases in temperature by 50°C, what is the mass of the silver? The specific heat of silver is 0.24 J/g°C

Multiple Choice

What variable is the number 50?

An unknown mass of silver is heated with 1240 J of energy and increases in temperature by 50°C, what is the mass of the silver? The specific heat of silver is 0.24 J/g°C

ΔT

T_final

T_initial

Multiple Choice

What variable is the goal?

An unknown mass of silver is heated with 1240 J of energy and increases in temperature by 50°C, what is the mass of the silver? The specific heat of silver is 0.24 J/g°C

Multiple Choice

Select the derived equation to solve for the goal?

An unknown mass of silver is heated with 1240 J of energy and increases in temperature by 50°C, what is the mass of the silver? The specific heat of silver is 0.24 J/g°C

$Q=mc\Delta T$

$\Delta T=\frac{Q}{mc}$

$m=\frac{Q}{c\Delta T}$

$c=\frac{Q}{m\Delta T}$

Multiple Choice

Solve:

An unknown mass of silver is heated with 1240 J of energy and increases in temperature by 50°C, what is the mass of the silver? The specific heat of silver is 0.24 J/g°C

15 000 g Ag

300 000 g Ag

6 g Ag

100 g Ag

Multiple Choice

What variable is the number 6500?

A substance with unknown specific heat and mass of 250 grams is heated with 6500 J of energy. If the initial temperature was 22°C and the final was 72°C. What is the specific heat of the substance?

Multiple Choice

What variable is the number 250?

Multiple Choice

What variable is the number 72?

T_final

T_initial

ΔT

Multiple Choice

What variable is the number 22?

T_final

T_initial

ΔT

Multiple Choice

What variable is the goal?

Multiple Choice

Select the derived equation to solve for the goal?

$Q=mc\Delta T$

$c=\frac{\Delta T}{mQ}$

$c=\frac{mQ}{\Delta T}$

$c=\frac{Q}{m\Delta T}$

Multiple Choice

Solve:

0.52 J/g°C

0.52 cal/g°C

0.27 J/g°C

0.27 cal/g°C

Multiple Choice

What variable is the number 53?

An aqueous reaction releases 2000 J of energy into 53 grams of water at 22°C. What is the final temperature?

Assume the specific heat of solution is 4.18 J/g°C.

Multiple Choice

What variable is the number 2000?

An aqueous reaction releases 2000 J of energy into 53 grams of water at 22°C. What is the final temperature?

Assume the specific heat of solution is 4.18 J/g°C.

Multiple Choice

What variable is the number 4.18?

An aqueous reaction releases 2000 J of energy into 53 grams of water at 22°C. What is the final temperature?

Assume the specific heat of solution is 4.18 J/g°C.

Multiple Choice

What variable is the number 22?

An aqueous reaction releases 2000 J of energy into 53 grams of water at 22°C. What is the final temperature?

Assume the specific heat of solution is 4.18 J/g°C.

T_initial

T_final

ΔT

Multiple Choice

What variable is the goal?

An aqueous reaction releases 2000 J of energy into 53 grams of water at 22°C. What is the final temperature?

Assume the specific heat of solution is 4.18 J/g°C.

T_initial

T_final

ΔT

Multiple Choice

Select the derived equation to solve for the goal?

An aqueous reaction releases 2000 J of energy into 53 grams of water at 22°C. What is the final temperature?

Assume the specific heat of solution is 4.18 J/g°C.

$T_f=\frac{Q}{mc}+T_i$

$T_f=\frac{Q}{mc}-T_i$

$T_f=\frac{Q}{mc-T_i}$

$T_f=\frac{Q}{mc+T_i}$

Multiple Choice

Solve:

An aqueous reaction releases 2000 J of energy into 53 grams of water at 22°C. What is the final temperature?

Assume the specific heat of solution is 4.18 J/g°C.

22°C

31°C

9°C

13°C

49°C

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