Heat Capacity and Specific Heat Flashcards - Physical Chemistry

Question

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Answer

Use the equation:

$q=mC\Delta T$

We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature $\Delta T$ , we can solve for .

$C = \frac{q}{m\Delta T} = \frac{2000J}{(50g)(10^{\circ} C)} = 4.0\frac{J}{g^{\circ} C}$

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Question

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?

Answer

Recall that the formula for specific heat is $q=mc\Delta T$ . Rearranging the equation for specific heat (c) yields $c=\frac{q}{m\Delta T}=\frac{-84J}{2.5g(-74.9^{\circ}C)}=0.449\frac{J}{{g\cdot ^{\circ}C}}$

Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and $\Delta T$ .

Compare your answer with the correct one above

Question

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Answer

Use the equation:

$q=mC\Delta T$

We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature $\Delta T$ , we can solve for .

$C = \frac{q}{m\Delta T} = \frac{2000J}{(50g)(10^{\circ} C)} = 4.0\frac{J}{g^{\circ} C}$

Compare your answer with the correct one above

Question

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?

Answer

Recall that the formula for specific heat is $q=mc\Delta T$ . Rearranging the equation for specific heat (c) yields $c=\frac{q}{m\Delta T}=\frac{-84J}{2.5g(-74.9^{\circ}C)}=0.449\frac{J}{{g\cdot ^{\circ}C}}$

Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and $\Delta T$ .

Compare your answer with the correct one above

Question

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Answer

Use the equation:

$q=mC\Delta T$

We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature $\Delta T$ , we can solve for .

$C = \frac{q}{m\Delta T} = \frac{2000J}{(50g)(10^{\circ} C)} = 4.0\frac{J}{g^{\circ} C}$

Compare your answer with the correct one above

Question

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?

Answer

Recall that the formula for specific heat is $q=mc\Delta T$ . Rearranging the equation for specific heat (c) yields $c=\frac{q}{m\Delta T}=\frac{-84J}{2.5g(-74.9^{\circ}C)}=0.449\frac{J}{{g\cdot ^{\circ}C}}$

Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and $\Delta T$ .

Compare your answer with the correct one above

Question

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Answer

Use the equation:

$q=mC\Delta T$

We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature $\Delta T$ , we can solve for .

$C = \frac{q}{m\Delta T} = \frac{2000J}{(50g)(10^{\circ} C)} = 4.0\frac{J}{g^{\circ} C}$

Compare your answer with the correct one above

Question

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?

Answer

Recall that the formula for specific heat is $q=mc\Delta T$ . Rearranging the equation for specific heat (c) yields $c=\frac{q}{m\Delta T}=\frac{-84J}{2.5g(-74.9^{\circ}C)}=0.449\frac{J}{{g\cdot ^{\circ}C}}$

Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and $\Delta T$ .

Compare your answer with the correct one above

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Heat Capacity and Specific Heat - Physical Chemistry

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Use the equation: We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature , we can solve for .

A sample of an unknown metal at is immersed in water and is allowed to reach equilibrium. If final temperature of the system is and of energy are released, what is the identity of the metal?

Recall that the formula for specific heat is . Rearranging the equation for specific heat (c) yields Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and .

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Use the equation: We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature , we can solve for .

A sample of an unknown metal at is immersed in water and is allowed to reach equilibrium. If final temperature of the system is and of energy are released, what is the identity of the metal?

Recall that the formula for specific heat is . Rearranging the equation for specific heat (c) yields Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and .

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Use the equation: We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature , we can solve for .

A sample of an unknown metal at is immersed in water and is allowed to reach equilibrium. If final temperature of the system is and of energy are released, what is the identity of the metal?

Recall that the formula for specific heat is . Rearranging the equation for specific heat (c) yields Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and .

What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?

Use the equation: We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample , and the change in temperature , we can solve for .

A sample of an unknown metal at is immersed in water and is allowed to reach equilibrium. If final temperature of the system is and of energy are released, what is the identity of the metal?

Recall that the formula for specific heat is . Rearranging the equation for specific heat (c) yields Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and .

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?

A sample of an unknown metal at $100^\circ C$ is immersed in water and is allowed to reach equilibrium. If final temperature of the system is $25.1^\circ C$ and of energy are released, what is the identity of the metal?