Question 1

When 49.5 J of heat was transferred to 7.3 g iron at 22°C,the temperature of iron increases to 37°C.What is the specific heat of iron in J/g∙°C?

Accepted Answer

The answer of When 49.5 J of heat was transferred...

Question 2

Suppose it took 108 joules of energy to raise a bar of gold from 25.0°C to 29.7°C.Given that the specific heat capacity of gold is 
,what is the mass (in grams)of the bar of gold?

Accepted Answer

The answer of Suppose it took 108 joules of energy...

Question 3

What is the specific heat (J/g∙°C)of a metal object whose temperature increases by 3.0°C when 17.5 g of metal was heated with 38.5 J?

Accepted Answer

The formula for calculating specific heat is:

Specific heat = (energy absorbed)/(mass x change in temperature)

We are given:
Energy absorbed (q) = 38.5 J
Mass (m) = 17.5 g
Change in temperature (ΔT) = 3.0°C

Plugging these values into the formula, we get:

Specific heat = (38.5 J)/(17.5 g x 3.0°C)
Specific heat = 0.73 J/g∙°C

Therefore, the answer is C) 0.73.

Question 4

The temperature of 390 kelvin is warmer than which one of the following temperatures?

Accepted Answer

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Question 5

A 15.0 gram lead ball at 25.0°C was heated with 40.5 joules of heat.Given the specific heat of lead is 0.128 J/g∙°C,what is the final temperature of the lead?

Accepted Answer

The answer of A 15.0 gram lead ball at 25.0°C...

Question 6

How many Calories are in 575.0 calories?

Accepted Answer

The answer of How many Calories are in 575.0 calories?
...

Question 7

From the following list of substances and heat capacities,choose the one that will have the lowest temperature after absorbing 100.0 kJ of heat.Assume identical masses of each substance start at the same initial temperature.

Accepted Answer

The substance with the lower heat capacity will experience a greater increase in temperature for a given amount of heat. Therefore, the substance with the higher heat capacity will experience a smaller increase in temperature for the same amount of heat. In this case, we want the substance that will have the lowest temperature after absorbing 100.0 kJ of heat. Since water has the highest heat capacity of the given choices, it will experience the smallest increase in temperature and therefore have the lowest final temperature.

Question 8

What is the value of 23°C on the Fahrenheit scale?

Accepted Answer

To convert Celsius to Fahrenheit, use the formula F = C * 9/5 + 32. For 23°C, it's 23 * 9/5 + 32 = 73.4, which rounds to 73.

Question 9

What is the value of -25°C on the Kelvin scale?

Accepted Answer

The answer of What is the value of -25°C on...

Question 10

Given the table of specific heat values below,what is the identity of a 26.2 g metal sample that increases by 8.5°C when 100.0 J of energy is absorbed?

Accepted Answer

Using the formula Q = mCΔT, where Q is the amount of energy absorbed, m is the mass of the metal, C is the specific heat, and ΔT is the change in temperature, we can calculate the specific heat of the metal sample:

C = Q / (mΔT) = 100 J / (26.2 g × 8.5 °C) = 0.456 J/g°C

Comparing this value to the specific heat values in the table, we see that the closest match is iron (Fe) with a specific heat of 0.449 J/g°C. Therefore, the identity of the metal sample is likely Fe.

Question 11

How much heat (kJ)is absorbed by 948.0 g of water in order for the temperature to increase from 
To

Accepted Answer

Using the equation Q = m*c*∆T, where Q is the heat absorbed/released, m is the mass of the substance, c is the specific heat capacity of the substance, and ∆T is the change in temperature, we can calculate the heat absorbed by 948.0 g of water:

Q = m*c*∆T = 948.0 g * 4.184 J/g°C * (21.8°C - 11.0°C)
Q = 29,706.14 J = 29.70 kJ

Therefore, the heat absorbed by the water is 29.7 kJ (choice D).

Question 12

Given the table of specific heat values below,what is the identity of a 10.0 g metal sample that increases by 
When 
Of energy is absorbed?

Accepted Answer

The answer of Given the table of specific heat values...

Question 13

What is the value of 783 K in units of °C?

Accepted Answer

To convert from Kelvin to Celsius, subtract 273. Therefore, 783 K - 273 = 510 °C. The correct answer is (C).

Question 14

How many grams of water when supplied with 
Of heat will gain a temperature of 5.2°C?

Accepted Answer

The answer of How many grams of water when supplied...

Question 15

How much heat (kJ)is needed to raise the temperature of 100.0 grams of water from 25.0°C to 
?

Accepted Answer

The answer of How much heat (kJ)is needed to raise...

Question 16

What is the final temperature of 25.0 grams of water at 22.0°C after it absorbs 
Of heat?

Accepted Answer

We can use the formula q = m*c*ΔT, where q is the heat absorbed by the water, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature. Solving for ΔT, we get:

ΔT = q / (m*c)

Plugging in the given values, we get:

ΔT = 11000 J / (25.0 g * 4.18 J/(g°C))
ΔT = 104.9 °C

Therefore, the final temperature of the water is:

Tf = Ti + ΔT
Tf = 22.0°C + 104.9°C
Tf = 126.9°C

However, water can only exist as a liquid up to its boiling point, which is 100°C at standard pressure. Therefore, the final temperature of the water will be the boiling point of water (100°C).

Question 17

How many joules are in 55.2 calories?

Accepted Answer

The answer of How many joules are in 55.2 calories?
...

Question 18

Consider the following specific heats of metals.
Metal Specific Heat (J/g∙°C)
Aluminum 0.903
Copper 0.385
Gold 0.128
Iron 0.449
Silver 0.235
If the same amount of heat is added to 50.0 g samples of each of the metals,which are all at the same temperature,which metal will reach the highest temperature?

Accepted Answer

The metal with the lowest specific heat will experience the highest temperature rise when the same amount of heat is added to it. Therefore, we need to find the metal with the lowest specific heat. From the options given, gold has the lowest specific heat value of 0.128 J/g∙°C, which means it will experience the highest temperature rise when the same amount of heat is added. Therefore, the correct choice is C) gold.

Quiz 3: Matter and Energy

When 49.5 J of heat was transferred to 7.3 g iron at 22°C,the temperature of iron increases to 37°C.What is the specific heat of iron in J/g∙°C?

Suppose it took 108 joules of energy to raise a bar of gold from 25.0°C to 29.7°C.Given that the specific heat capacity of gold is ,what is the mass (in grams) of the bar of gold?

What is the specific heat (J/g∙°C) of a metal object whose temperature increases by 3.0°C when 17.5 g of metal was heated with 38.5 J?

The temperature of 390 kelvin is warmer than which one of the following temperatures?

A 15.0 gram lead ball at 25.0°C was heated with 40.5 joules of heat.Given the specific heat of lead is 0.128 J/g∙°C,what is the final temperature of the lead?

How many Calories are in 575.0 calories?

From the following list of substances and heat capacities,choose the one that will have the lowest temperature after absorbing 100.0 kJ of heat.Assume identical masses of each substance start at the same initial temperature.

What is the value of 23°C on the Fahrenheit scale?

What is the value of -25°C on the Kelvin scale?

Given the table of specific heat values below,what is the identity of a 26.2 g metal sample that increases by 8.5°C when 100.0 J of energy is absorbed?

How much heat (kJ) is absorbed by 948.0 g of water in order for the temperature to increase from To

Given the table of specific heat values below,what is the identity of a 10.0 g metal sample that increases by When Of energy is absorbed?

What is the value of 783 K in units of °C?

How many grams of water when supplied with Of heat will gain a temperature of 5.2°C?

How much heat (kJ) is needed to raise the temperature of 100.0 grams of water from 25.0°C to ?

What is the final temperature of 25.0 grams of water at 22.0°C after it absorbs Of heat?

How many joules are in 55.2 calories?