Question 1

Which of the following best describes the relationship between heat ($q$) and temperature change ($\Delta T$) for an object?

Accepted Answer

Heat is directly proportional to temperature change.

Question 2

If the temperature of a water bath goes from 25 K to 50 K, what can be said about the amount of heat absorbed, assuming all other factors remain constant?

Accepted Answer

It will double.

Question 3

Which formula correctly represents the calculation of specific heat capacity?

Accepted Answer

$q = m \cdot c \cdot \Delta T$

Question 4

A sample of copper absorbs 3.53 kJ of heat, which increases its temperature by 25 $^\circ$C. What is the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g·$^\circ$C?

Accepted Answer

0.367 kg

Question 5

Which compound would show the greatest temperature change upon absorbing 250 J of heat, based on the given specific heat capacities?

Accepted Answer

250.0 g Cu

Question 6

If 15.7 g of silver raises its temperature by 17.2 $^\circ$C when it absorbs 6845.5 J of heat, what is its molar heat capacity?

Accepted Answer

$273.1 \cdot 10^{-3}$ J/mol·$^\circ$C

Question 7

How much heat (in kJ) is released when 120.0 g H$_2$O goes from 90 $^\circ$C to 45 $^\circ$C? The specific heat capacity of H$_2$O is 4.184 J/g·$^\circ$C.

Accepted Answer

$-22.5936$ kJ

Question 8

A 50.0 g heated metal is placed into an insulated beaker containing 822.5 g of water. Once the metal heats up, the final temperature of the water is 32.08 $^\circ$C. If the metal gains 14.55 kJ of energy, what is the initial temperature of the water? The specific heat capacity of copper is 4.184 J/g·$^\circ$C.

Accepted Answer

80.3 $^\circ$C

Question 9

Which of the following statements about molar heat capacity is correct?

Accepted Answer

It is the amount of heat required to change the temperature of 1 mole of substance by 1 K.

Question 10

Which of the following would result in the largest temperature increase for a given amount of heat absorbed?

Accepted Answer

A substance with a low specific heat capacity.

Question 11

If 100 g of ethanol (specific heat capacity = 2.460 J/g·$^\circ$C) absorbs 500 J of heat, what is the temperature change?

Accepted Answer

$\Delta T = 2.04^\circ$C

Question 12

Which of the following is NOT a correct unit for specific heat capacity?

Accepted Answer

J/K·g

Question 13

A 250 g sample of aluminum (specific heat capacity = 0.900 J/g·$^\circ$C) is heated from 20 $^\circ$C to 50 $^\circ$C. How much heat is absorbed?

Accepted Answer

$q = 6,750$ J

Question 14

Which of the following scenarios best illustrates the concept of heat capacity in a real-world context?

Accepted Answer

A metal spoon heating up quickly in hot soup.

Question 15

If the specific heat capacity of a substance is high, what does this imply about its ability to change temperature?

Accepted Answer

It will require more heat to change its temperature.

Question 16

Which equation would you use to calculate the amount of heat released or absorbed by a substance?

Accepted Answer

$q = m \cdot c \cdot \Delta T$

Heat Capacity and Specific Heat in GOB Chemistry

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