Specific Heat - Page 2
Questions
- How do the specific heats of metals compare with water?
- An object with a mass of #4 kg#, temperature of #265 ^oC#, and a specific heat of #12 (KJ)/(kg*K)# is dropped into a container with #39 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- An object with a mass of #100 g# is dropped into #500 mL# of water at #0^@C#. If the object cools by #50 ^@C# and the water warms by #4 ^@C#, what is the specific heat of the material that the object is made of?
- An object with a mass of #1 kg#, temperature of #350 ^oC#, and a specific heat of #14 J/(kg*K)# is dropped into a container with #16 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- An object with a mass of #18 g# is dropped into #400 mL# of water at #0^@C#. If the object cools by #150 ^@C# and the water warms by #12 ^@C#, what is the specific heat of the material that the object is made of?
- What is the specific heat of a substance that absorbs #2.5*10^3# joules of heat when a sample of #1 * 10^4# g of the substance increases in temperature from 10°C to 80°C?
- An object with a mass of #12 kg#, temperature of #125 ^oC#, and a specific heat of #32 (KJ)/(kg*K)# is dropped into a container with #35 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- Which will normally warm faster: a black pot of cold water or a silvered pot of cold water? Which will cool faster?
- An object with a mass of #12 kg#, temperature of #175 ^oC#, and a specific heat of #32 J/(kg*K)# is dropped into a container with #35 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- What is the specific heat of ice in j/gc?
- How much energy is needed to change the temperature of 95.4g of nickel from 22°C to 32°C? Is the energy absorbed or released?
- An object with a mass of #100 g# is dropped into #500 mL# of water at #0^@C#. If the object cools by #20 ^@C# and the water warms by #4 ^@C#, what is the specific heat of the material that the object is made of?
- The specific heat of concrete is greater than that of soil. Given this fact, would you expect a major-league baseball field or the parking lot that surrounds it to cool off more in the evening following a sunny day?
- An object with a mass of #3 kg#, temperature of #210 ^oC#, and a specific heat of #24 J/(kg*K)# is dropped into a container with #36 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- An object with a mass of #2 kg#, temperature of #331 ^oC#, and a specific heat of #18 (KJ)/(kg*K)# is dropped into a container with #37 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- An object with a mass of #6 kg#, temperature of #160 ^oC#, and a specific heat of #9 J/(kg*K)# is dropped into a container with #27 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- An object with a mass of #6 kg#, temperature of #50 ^oC#, and a specific heat of #4 J/(kg*K)# is dropped into a container with #24 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- Determine the specific heat of unknown metal from the fact that 6.40 * 10-2kj are needed to raise the temperature of 15g of unknown metal from 22 degrees Celsius to 33 degrees Celsius?
- How do you calculate specific heat capacity given heat flow, mass and temperature change?
- An object with a mass of #16 kg#, temperature of #240 ^oC#, and a specific heat of #6 J/(kg*K)# is dropped into a container with #48 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?