Specific Heat - Page 6
Questions
- An object with a mass of #160 g# is dropped into #880 mL# of water at #0^@C#. If the object cools by #120 ^@C# and the water warms by #12 ^@C#, what is the specific heat of the material that the object is made of?
- An object with a mass of #125 g# is dropped into #750 mL# of water at #0^@C#. If the object cools by #70 ^@C# and the water warms by #3 ^@C#, what is the specific heat of the material that the object is made of?
- An object with a mass of #24 kg#, temperature of #210 ^oC#, and a specific heat of #8 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?
- What is the specific heat of ice at #0^oC#?
- An insulated beaker contains 300 g of water at #30^o C #. Water at #100^o C# is added until the temperature of the mixture reaches #50^o C#. The specific heat capacity of water is 4.2 J/#(g^o C)#. How much water is added?
- An object with a mass of #4 g# is dropped into #650 mL# of water at #0^@C#. If the object cools by #12 ^@C# and the water warms by #30 ^@C#, what is the specific heat of the material that the object is made of?
- When calculating the mass of a Uranium-235 nucleus, can we just subtract the mass of the electrons from the given mass of a Uranium-235 atom?
- Solid iron a specific heat of 0.444 J/g°C. If 75 calories of energy were removed from a piece of iron, and the temperature of the iron went from 21.4°C to -25.2°C, what was the mass of the iron?
- An object with a mass of #4 kg#, temperature of #240 ^oC#, and a specific heat of #5 J/(kg*K)# is dropped into a container with #32 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 #30 g# is dropped into #50 mL# of water at #0^@C#. If the object cools by #20 ^@C# and the water warms by #80 ^@C#, what is the specific heat of the material that the object is made of?
- An object with a mass of #180 g# is dropped into #660 mL# of water at #0^@C#. If the object cools by #36 ^@C# and the water warms by #3 ^@C#, what is the specific heat of the material that the object is made of?
- How many grams of formaldehyde are needed to produce enough heat in a combustion reaction to change 10.00g of ice to steam at 100 degrees C?
- An object with a mass of #2 kg#, temperature of #150 ^oC#, and a specific heat of #24 J/(kg*K)# is dropped into a container with #18 L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?
- If it takes 41.72 joules to heat a piece of gold weighing 18.69 g from 10.0°C to 27.0°C, what is the specific heat of the gold?
- How do specific heats of metal compare to that of water?
- An object with a mass of #40 g# is dropped into #660 mL# of water at #0^@C#. If the object cools by #72 ^@C# and the water warms by #3 ^@C#, what is the specific heat of the material that the object is made of?
- What is the specific heat capacity of silver atom, if #"386 g"# of #"Ag"# has a heat capacity of #"91.5 J/"^@ "C"#?
- The specific heat of copper is 0.385 J/g #*# °C. How would you calculate the amount of heat needed to raise the temperature of 0.75 g of copper from 7°C to 29°C?
- An object with a mass of #1 kg#, temperature of #350 ^oC#, and a specific heat of #6 J/(kg*K)# is dropped into a container with #28 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 #150 g# is dropped into #500 mL# of water at #0^@C#. If the object cools by #60 ^@C# and the water warms by #9 ^@C#, what is the specific heat of the material that the object is made of?