A lead block with a mass of 46.5 g at a temperature of 76.98 degrees celsius...
A lead block with a mass of 46.5 g at a temperature of 76.98 degrees celsius was placed into a calorimeter containing 100.0 mL of water at a temperature of 20.6 degrees celsius. What is the equilibrium temperature if the specific heat of water is 4.184 J/g and the specific heat of lead is 0.158 J/gdegreeC?
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A lead block with a mass of 46.5 g at a temperature of 76.98
degrees celsius...
A metal sample weighing 24.000 g is heated to 100.0 degrees celsius and then transferred into a calorimeter containing 3...
A metal sample weighing 24.000 g is heated to 100.0 degrees celsius and then transferred into a calorimeter containing 30.0 mL of water at a temperature of 22.8 degrees celsius. If the specific heat of the metal is 0.105 J/g*C, what is the final temperature of the metal sample plus water?
Please help how to solve this question An unknown metal weighting 13.11 g at a temperature...
Please help how to solve this question An unknown metal weighting 13.11 g at a temperature of 81.0 degrees Celius is place in a calorimeter containing 25.0 mL of water at a temperature of 25.0 degrees Celsius. The final equilibrium temperature is 30.0 degrees Celius. What s the specific heat of the metal? The specific heat of water is 4.184 J/g-C. Assume the density of water is 1.00g/mL and that there is no heat lost or gained by the calorimeter.
A block of an alloy of mass 33.0 g and at a temperature of 295.58 K...
A block of an alloy of mass 33.0 g and at a temperature of 295.58 K is placed in a calorimeter containing 50.0 g of water at 344.84 K. If the final temperature of the alloy and water is 326.33 K, calculate the specific heat (in J/g/K) of the metal. The specific heat of water is 4.184 J/g/K. Express your answer to three significant figures in scientific notation.
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed...
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed in 400 g of water at 25 degrees Celsius? The specific heat capacity of iron 0.45 J/g*K and the specific heat capacity of water is 4.184 J/g*K.
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed...
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed in 400 g of water at 25 degrees Celsius? The specific heat capacity of iron 0.45 J/g*K and the specific heat capacity of water is 4.184 J/g*K
A hot lump of 32.3g of Copper at an initial temperature of 96.5 degrees Celsius in...
A
hot lump of 32.3g of Copper at an initial temperature of 96.5
degrees Celsius in 50mL H2O initially at 25.0 degrees Celsius and
allowed to reach thermal equilibrium. What is the final temperature
of the copper and water, given that the specific hear is 0.385J/g°C
and the specific heat of water is 4.184J/g°C?
4. A hot lump of 41.3 g of copper at an initial temperature of 94.8 °C is placed in 50.0 mL H2O initially at 25.0 °C...
A 69.62 g block of lead is heated to 99.48ºC and is placed into a coffee-cup...
A 69.62 g block of lead is heated to 99.48ºC and is placed into a coffee-cup calorimeter filled with 75.67 g of water initially at 22.07ºC. The final temperature was measured as 24.58ºC. The calorimeter heat capacity is 1.860 J/ºC and the specific heat of water is 4.184 J/ g ºC. Based on this information, what is the specific heat of lead? a.0.1473 J/ g ºC b.0.1481 J/ g ºC c.0.1523 J/ g ºC d.0.1533 J/ g ºC e.0.2109 J/...
A piece of lead with amass of 1.75 kg and a temperature of 95.0 degrees Celsius...
A piece of lead with amass of 1.75 kg and a temperature of 95.0 degrees Celsius is added to a 225 g of water at 23 degrees Celsius. The water is contained in an aluminium cup which has a mass of 75.0 g. Determine the final equilibrium temperature of the lead, water, and aluminium cup if no heat is lost to the surroundings.
A dish containing 145 g of water at 54.0 degrees Celsius is put in a refrigerator...
A dish containing 145 g of water at 54.0 degrees Celsius is put in a refrigerator to cool. It is removed when the temperature ofthe water is 5.50 degrees Celsius. (Specific heat H2O(l)=4.184 j/gC. a) how much heat (in KJ) does the water lose? b) Describe how the entropy of the system changes in this process?
A 10.95 g sample of lead at 88.0°C was placed into a styrofoam cup calorimeter which...
A 10.95 g sample of lead at 88.0°C was placed into a styrofoam cup calorimeter which contained 15 mL of water at 22.0°C. The final temperature in the calorimeter reached 23.5°C. Calculate the specific heat of lead. The specific heat of water is 4.184 J/g°C.
A
hot lump of 32.3g of Copper at an initial temperature of 96.5
degrees Celsius in 50mL H2O initially at 25.0 degrees Celsius and
allowed to reach thermal equilibrium. What is the final temperature
of the copper and water, given that the specific hear is 0.385J/g°C
and the specific heat of water is 4.184J/g°C?
4. A hot lump of 41.3 g of copper at an initial temperature of 94.8 °C is placed in 50.0 mL H2O initially at 25.0 °C...
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