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A solution is made by mixing 285.0 ml. of ethanol initially at 11.7°C with 285.0 ml....
A solution is made by mixing 285.0 mL of ethanol initially at 11.7 C with 285.0 mL of water initially at 21.9 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g.°C and the specific heat of water is 4.184 J/g °C. Ti = "C The specific heat capacities for several substances...
A solution is made by mixing 244.0 mL 244.0 mL of ethanol initially at 13.0 ∘ C 13.0 ∘C with 244.0 mL 244.0 mL of water initially at 21.4 ∘ C 21.4 ∘C . What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL 0.789 g/mL and the density of water is 1.00 g/mL 1.00 g/mL . The specific heat of ethanol is 2.46 J/g·°C 2.46 J/g·°C and the...
A solution is made by mixing 207.0 mL of ethanol initially at 14.7 ∘C with 207.0 mL of water initially at 23.9 ∘C . What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL . The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C
A solution is made by mixing 223.0 mL of ethanol initially at15.3 ∘C with 223.0 mL of water initially at 21.1 ∘C What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g⋅°C and the specific heat of water is 4.184 J/g⋅°C. Tf= ∘C
An irregular lump of an unknown metal has a measured density of 3.84 g/mL. The metal is heated to a temperature of 161 °C and placed in a graduated cylinder filled with 25.0 mL of water at 25.0 °C. After the system has reached thermal equilibrium, the volume in the cylinder is read at 33.7 mL, and the temperature is recorded as 37.4 °C. What is the specific heat of the unknown metal sample? Assume no heat is lost to...
1. A 110.4 g110.4 g sample of a substance is initially at 20.1 °C20.1 °C . After absorbing 335 cal335 cal of heat, the temperature of the substance increases to 67.6 °C67.6 °C . What is the specific heat (SH)(SH) of the substance? 2. When 165.0165.0 J of heat are added to a 15.015.0 g sample of mercury the final temperature of the mercury is recorded as 63.063.0 °C. The metal has a specific heat of 0.13950.1395 J/(g·°C). 3. A...
3. with ethanol. The morning begins at 25°C, an a the lake that is filled with water, how much le Suppose all the water in a 1.000.000-L lake is replaced with ethanol. The morning the temperature quickly rises to 35°C. Compared with the lake that is filled with water heat would the lake filled with ethanol be able to led with ethanol be able to absorb? The density of ethanol is 0.789 g/mL and t density of water is 1.00...
22.7 mL of ethanol (density =0.789 g/mL) initially at 8.4 ?C is mixed with 30.5 mL of water (density = 1.0 g/mL) initially at 23.8 ?C in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the mixture?
If 46.9 mL of ethanol (density = 0.789 g/mL) initially at 7.2°C is mixed with 45.4 mL of water (density = 1.0 g/mL) initially at 28.5°C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?
If 55.0 mL of ethanol (density = 0.789 g/mL ) initially at 6.0 ∘ C is mixed with 55.0 mL of water (density = 1.0 g/mL ) initially at 28.6 ∘ C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost? ( C EtOH =2.42J/(g⋅ ∘ C). ) Express the temperature in degrees Celsius to three significant figures.