Question 1

The energy associated with a stretched spring is called _____.

Accepted Answer

The energy associated with a stretched spring is an example of potential energy, since it is stored energy that can be converted into kinetic energy if the spring is released. Choices A through D do not accurately describe the energy associated with a stretched spring.

Question 2

Exactly 149.6 J will raise the temperature of 10.0 g of a metal from 25.0 °C to 60.0 °C.What is the specific heat capacity of the metal?

Accepted Answer

The specific heat capacity (c) is given by: 
c = Q/(mΔT) 
where Q is the amount of heat absorbed or released, m is the mass of the substance, and ΔT is the change in temperature. Substituting the given values: 
c = 149.6 J/(10.0 g x (60.0 °C - 25.0 °C)) 
c = 0.427 J/(g · °C) 
Therefore, the specific heat capacity of the metal is 0.427 J/(g · °C) which is closest to option A).

Question 3

If 46.1 g of copper at 11.6 °C is placed in 85.0 g of water at 72.4 °C,what is the final temperature of the mixture? The specific heat capacities of copper and water are 0.385 J/g ⋅ K and 4.184 J/g ⋅ K,respectively.

Accepted Answer

The final temperature of the mixture can be found by setting the heat gained by the copper equal to the heat lost by the water, using the formula $q = mc\Delta T$, where $q$ is the heat transferred, $m$ is the mass, $c$ is the specific heat capacity, and $\Delta T$ is the change in temperature. Solving for the final temperature gives approximately 69.5 °C.

Question 4

How much energy is gained by copper when 68.4 g of copper is warmed from 13.4 °C to 78.4 °C? The specific heat capacity of copper is 0.385 J/(g·°C).

Accepted Answer

We can use the formula Q = mcΔT, where Q is the energy gained, m is the mass of copper, c is the specific heat capacity of copper, and ΔT is the change in temperature.

Plugging in the given values, we get:

Q = (68.4 g)(0.385 J/(g·°C))(78.4 °C - 13.4 °C)
Q = 1.71 × 10^3 J

Therefore, the energy gained by copper is 1.71 × 10^3 J, which corresponds to choice D.

Question 5

It is relatively easy to change the temperature of a substance that

Accepted Answer

Substances with a low specific heat capacity require less energy to change their temperature, making it easier to heat up or cool down compared to substances with a high specific heat capacity.

Question 6

Calculate the energy in the form of heat (in kJ)required to convert 325 grams of liquid water at 20.0 °C to steam at 115 °C.Assume that no energy in the form of heat is transferred to the environment.(Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: liquid water = 4.184 J/g⋅K,steam = 1.92 J/g⋅K)

Accepted Answer

The answer of Calculate the energy in the form of...

Question 7

Which of the following processes will result in the lowest final temperature of the metal-water mixture at when thermal equilibrium is reached? The specific heat capacity of iron is 0.449 J/(g·°C).The specific heat capacity of water is 4.184 J/(g·°C).

Accepted Answer

The final temperature is lowest when the water mass is highest because water has a higher specific heat capacity than iron, meaning it can absorb more heat without a large temperature increase. Option B has the highest water volume (100 mL), leading to the lowest final temperature.

Question 8

How much energy is needed to convert 50.8 g of ice at 0.00 °C to liquid water at 75.0 °C? Specific heat capacity (ice)= 2.10 J/g °C
Specific heat capacity (liquid water)= 4.18 J/g °C
Heat of fusion = 333 J/g
Heat of vaporization = 2258 J/g

Accepted Answer

The answer of How much energy is needed to convert...

Question 9

Which of these physical changes would require the release of energy?

Accepted Answer

Freezing a liquid into a solid requires the release of energy in the form of heat. This process is exothermic, meaning it releases heat to the surroundings.

Question 10

If 35.0 g H₂O at 22.7 °C is combined with 65.0 g H₂O at 87.5 °C,what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.

Accepted Answer

The answer of If 35.0 g H₂O at 22.7 °C...

Question 11

Which one of the following statements is INCORRECT?

Accepted Answer

Kinetic energy is the energy that results from an object's motion, not position. Potential energy is the energy that results from an object's position.

Question 12

Which of the following is an endothermic process?

Accepted Answer

An endothermic process is one in which the system absorbs energy from its surroundings. When work is done on the system by the surroundings, it means energy is being transferred to the system, making it an endothermic process.

Question 13

A 18.6-g piece of gold (s = 0.129 J/(g·°C)),initially at 285.4°C,is added to 147.2 g of a liquid,initially at 27.9°C,in an insulated container.The final temperature of the metal-liquid mixture at equilibrium is 28.9°C.What is the identity of the liquid? Neglect the heat capacity of the container.

Accepted Answer

First, we need to use the formula for calculating the heat released or absorbed during a temperature change:
q = m * s * ΔT
where q is the heat released or absorbed, m is the mass of the substance, s is its specific heat capacity, and ΔT is the temperature change.

For the gold piece, the heat released (since it is cooling down) is:
q1 = 18.6 g * 0.129 J/g°C * (285.4°C - 28.9°C) = -108356 J

For the liquid, the heat absorbed (since it is warming up) is:
q2 = 147.2 g * s * (28.9°C - 27.9°C)

At equilibrium, the total heat released must be equal to the total heat absorbed:
q1 = -q2
-108356 J = -147.2 g * s * (28.9°C - 27.9°C)
s = 4.18 J/(g·°C)

This value of specific heat capacity matches with that of water. Therefore, the liquid in the container is most likely water.

Question 14

Heat capacity is defined as

Accepted Answer

Heat capacity is the amount of heat required to raise the temperature of a substance (regardless of its mass) by 1 K.

Question 15

The specific heat capacity of water(liquid)is 4.18 J/g⋅°C.What is the molar specific heat capacity of this substance? The molar mass of water is 18.01 g/mol.

Accepted Answer

The molar specific heat capacity can be calculated by multiplying the specific heat capacity by the molar mass. For water, this is 4.18 J/g⋅°C * 18.01 g/mol = 75.3 J/mol⋅°C.

Question 16

When 66.0 g of an unknown metal at 28.5 °C is placed in 83.0 g H₂O at 78.5 °C,the water temperature decreases to 75.9 °C.What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/g⋅K.

Accepted Answer

The specific heat capacity of the metal can be found using the principle of conservation of energy, where the heat lost by the water is equal to the heat gained by the metal. The formula to calculate the specific heat capacity ($c_m$) of the metal is derived from $q = mc\Delta T$, where $q$ is the heat transferred, $m$ is the mass, $c$ is the specific heat capacity, and $\Delta T$ is the change in temperature.Given:- Mass of water ($m_w$) = 83.0 g- Initial temperature of water ($T_{wi}$) = 78.5 °C- Final temperature of water ($T_{wf}$) = 75.9 °C- Mass of metal ($m_m$) = 66.0 g- Initial temperature of metal ($T_{mi}$) = 28.5 °C- Final temperature of metal ($T_{mf}$) = 75.9 °C (same as the final temperature of water)- Specific heat capacity of water ($c_w$) = 4.184 J/g⋅KFirst, calculate the heat lost by the water:$$q_w = m_w \cdot c_w \cdot (T_{wf} - T_{wi})$$$$q_w = 83.0 \cdot 4.184 \cdot (75.9 - 78.5)$$$$q_w = 83.0 \cdot 4.184 \cdot (-2.6)$$$$q_w = -900.5 \, \text{J} \, (\text{approximately})$$Since the heat lost by the water is equal to the heat gained by the metal:$$q_m = -q_w$$$$q_m = 900.5 \, \text{J}$$Now, calculate the specific heat capacity of the metal using the heat gained by the metal:$$q_m = m_m \cdot c_m \cdot (T_{mf} - T_{mi})$$$$900.5 = 66.0 \cdot c_m \cdot (75.9 - 28.5)$$$$c_m = \frac{900.5}{66.0 \cdot 47.4}$$$$c_m = \frac{900.5}{3128.4}$$$$c_m = 0.288 \, \text{J/g⋅K}$$Therefore, the specific heat capacity of the metal is approximately 0.29 J/g⋅K, which corresponds to choice B.

Question 17

If 50.0 g of benzene (C₆H₆)absorbs 2.71 kJ of energy in the form of heat at 25.0 °C,what is the final temperature of benzene? The specific heat capacity of benzene is 1.72 J/g ⋅ K.

Accepted Answer

The answer of If 50.0 g of benzene (C₆H₆)absorbs 2.71...

Question 18

Specific heat capacity is

Accepted Answer

Specific heat capacity is defined as the quantity of heat (in joules) needed to change the temperature of 1.00 gram of a substance by 1 Kelvin (or 1 degree Celsius).

Question 19

A 170.0-g sample of metal at 83.00°C is added to 170.0 g of H₂O(l)at 15.00°C in an insulated container.The temperature rises to 18.16°C.Neglecting the heat capacity of the container,what is the specific heat capacity of the metal? The specific heat capacity of H₂O(l)is 4.18 J/(g·°C).

Accepted Answer

The specific heat capacity of the metal can be found using the principle of conservation of energy, which states that the heat lost by the metal will be equal to the heat gained by the water. The formula to calculate the specific heat capacity ($c_m$) of the metal is derived from $q = mc\Delta T$, where $q$ is the heat transferred, $m$ is the mass, $c$ is the specific heat capacity, and $\Delta T$ is the change in temperature.For the metal:$$q_m = m_m \cdot c_m \cdot (T_f - T_i)$$For the water (H₂O(l) is assumed to be water with a typo):$$q_w = m_w \cdot c_w \cdot (T_f - T_i)$$Given that the heat lost by the metal is equal to the heat gained by the water, and neglecting the heat capacity of the container:$$m_m \cdot c_m \cdot (T_f - T_i)_m = m_w \cdot c_w \cdot (T_f - T_i)_w$$Given:- $m_m = m_w = 170.0 \, g$- $c_w = 4.18 \, J/(g·°C)$- $T_{i,m} = 83.00°C$, $T_{i,w} = 15.00°C$, $T_f = 18.16°C$Substituting the given values:$$170.0 \cdot c_m \cdot (18.16 - 83.00) = 170.0 \cdot 4.18 \cdot (18.16 - 15.00)$$Solving for $c_m$:$$c_m = \frac{170.0 \cdot 4.18 \cdot (18.16 - 15.00)}{170.0 \cdot (18.16 - 83.00)}$$$$c_m = \frac{4.18 \cdot 3.16}{-64.84}$$$$c_m \approx 0.204 \, J/(g·°C)$$Therefore, the specific heat capacity of the metal is approximately 0.204 J/(g·°C).

Question 20

Many homes are heated using natural gas.The combustion of natural gas converts

Accepted Answer

The combustion of natural gas involves a chemical reaction that releases energy in the form of heat, which is then used to generate thermal energy for heating homes. This means that chemical potential energy is being converted into thermal energy.

Quiz 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

The energy associated with a stretched spring is called _____.

Exactly 149.6 J will raise the temperature of 10.0 g of a metal from 25.0 °C to 60.0 °C.What is the specific heat capacity of the metal?

If 46.1 g of copper at 11.6 °C is placed in 85.0 g of water at 72.4 °C,what is the final temperature of the mixture? The specific heat capacities of copper and water are 0.385 J/g ⋅ K and 4.184 J/g ⋅ K,respectively.

How much energy is gained by copper when 68.4 g of copper is warmed from 13.4 °C to 78.4 °C? The specific heat capacity of copper is 0.385 J/(g·°C) .

It is relatively easy to change the temperature of a substance that

Which of the following processes will result in the lowest final temperature of the metal-water mixture at when thermal equilibrium is reached? The specific heat capacity of iron is 0.449 J/(g·°C) .The specific heat capacity of water is 4.184 J/(g·°C) .

How much energy is needed to convert 50.8 g of ice at 0.00 °C to liquid water at 75.0 °C? Specific heat capacity (ice) = 2.10 J/g °C Specific heat capacity (liquid water) = 4.18 J/g °C Heat of fusion = 333 J/g Heat of vaporization = 2258 J/g

Which of these physical changes would require the release of energy?

If 35.0 g H₂O at 22.7 °C is combined with 65.0 g H₂O at 87.5 °C,what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.

Which one of the following statements is INCORRECT?

Which of the following is an endothermic process?

Heat capacity is defined as

The specific heat capacity of water(liquid) is 4.18 J/g⋅°C.What is the molar specific heat capacity of this substance? The molar mass of water is 18.01 g/mol.

When 66.0 g of an unknown metal at 28.5 °C is placed in 83.0 g H₂O at 78.5 °C,the water temperature decreases to 75.9 °C.What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/g⋅K.

If 50.0 g of benzene (C₆H₆) absorbs 2.71 kJ of energy in the form of heat at 25.0 °C,what is the final temperature of benzene? The specific heat capacity of benzene is 1.72 J/g ⋅ K.

Specific heat capacity is

A 170.0-g sample of metal at 83.00°C is added to 170.0 g of H₂O(l) at 15.00°C in an insulated container.The temperature rises to 18.16°C.Neglecting the heat capacity of the container,what is the specific heat capacity of the metal? The specific heat capacity of H₂O(l) is 4.18 J/(g·°C) .

Many homes are heated using natural gas.The combustion of natural gas converts

Quiz 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

The energy associated with a stretched spring is called _____.

Exactly 149.6 J will raise the temperature of 10.0 g of a metal from 25.0 °C to 60.0 °C.What is the specific heat capacity of the metal?

If 46.1 g of copper at 11.6 °C is placed in 85.0 g of water at 72.4 °C,what is the final temperature of the mixture? The specific heat capacities of copper and water are 0.385 J/g ⋅ K and 4.184 J/g ⋅ K,respectively.

How much energy is gained by copper when 68.4 g of copper is warmed from 13.4 °C to 78.4 °C? The specific heat capacity of copper is 0.385 J/(g·°C) .

It is relatively easy to change the temperature of a substance that

Which of the following processes will result in the lowest final temperature of the metal-water mixture at when thermal equilibrium is reached? The specific heat capacity of iron is 0.449 J/(g·°C) .The specific heat capacity of water is 4.184 J/(g·°C) .

How much energy is needed to convert 50.8 g of ice at 0.00 °C to liquid water at 75.0 °C? Specific heat capacity (ice) = 2.10 J/g °C Specific heat capacity (liquid water) = 4.18 J/g °C Heat of fusion = 333 J/g Heat of vaporization = 2258 J/g

Which of these physical changes would require the release of energy?

If 35.0 g H2O at 22.7 °C is combined with 65.0 g H2O at 87.5 °C,what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.

Which one of the following statements is INCORRECT?

Which of the following is an endothermic process?

Heat capacity is defined as

The specific heat capacity of water(liquid) is 4.18 J/g⋅°C.What is the molar specific heat capacity of this substance? The molar mass of water is 18.01 g/mol.

When 66.0 g of an unknown metal at 28.5 °C is placed in 83.0 g H2O at 78.5 °C,the water temperature decreases to 75.9 °C.What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/g⋅K.

If 50.0 g of benzene (C6H6) absorbs 2.71 kJ of energy in the form of heat at 25.0 °C,what is the final temperature of benzene? The specific heat capacity of benzene is 1.72 J/g ⋅ K.

Specific heat capacity is

A 170.0-g sample of metal at 83.00°C is added to 170.0 g of H2O(l) at 15.00°C in an insulated container.The temperature rises to 18.16°C.Neglecting the heat capacity of the container,what is the specific heat capacity of the metal? The specific heat capacity of H2O(l) is 4.18 J/(g·°C) .

Many homes are heated using natural gas.The combustion of natural gas converts

If 35.0 g H₂O at 22.7 °C is combined with 65.0 g H₂O at 87.5 °C,what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.

When 66.0 g of an unknown metal at 28.5 °C is placed in 83.0 g H₂O at 78.5 °C,the water temperature decreases to 75.9 °C.What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/g⋅K.

If 50.0 g of benzene (C₆H₆) absorbs 2.71 kJ of energy in the form of heat at 25.0 °C,what is the final temperature of benzene? The specific heat capacity of benzene is 1.72 J/g ⋅ K.

A 170.0-g sample of metal at 83.00°C is added to 170.0 g of H₂O(l) at 15.00°C in an insulated container.The temperature rises to 18.16°C.Neglecting the heat capacity of the container,what is the specific heat capacity of the metal? The specific heat capacity of H₂O(l) is 4.18 J/(g·°C) .