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a6f34c2c2eb8&attempt 1 Question 1 Volume Water 114.64 mL Initial Temperature of Water 60 °C Volume of...
4. A hot lump of 44.5 g of copper at an initial temperature of 60.7°C is placed in 50.0 mL H20 initially at 25.0°C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385J/gºC and the specific heat of water is 4.184 J/gºC? a. 23.7°C c. 27.7°C b. 25.7°C d. 29.7°C
1. 50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in a calorimeter also at 23.2°C. The final temperature was 33.1°C. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mlº', specific heat capacity=4.18 J g?K=) 2. When 5.00 g of NaOH(s) are added to 100 g of water (using the same calorimeter as...
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH" (aq) - H20 (1) is -56.2...
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
help 2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC. the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH(aq) → H20 (1) is -56.2...
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 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 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 Jig:"C and the specific heat of water is 4.184 J/g:°C. Ti = 30.7 "C Incorrect
If the temperature of 100.0 mL of water rises from 25.0°C to 32.0°C, how much heat was added? Assume the density of water is 1.00 g/mL and the specific heat capacity of the water is 4.184 J/g°C. Include units and use the correct number of significant figures. Define the terms "exothermic" and "endothermic". What is the sign of AH associated with these two terms? Exothermic: Endothermic
50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in a calorimeter also at 23.2°C. The final temperature was 33.1°C. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mL"', specific heat capacity= 4.18 J g'K:')