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50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in...
1. 50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°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 ml'', specific heat capacity = 4.18 Jg'K')
1. 50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°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...
1. A volume of water was heated to 81.76 °C and immediately added to 48.80 mL of water at 20.55 °C contained within a co...
1. A volume of water was heated to 81.76 °C and immediately added to 48.80 mL of water at 20.55 °C contained within a coffee cup calorimeter. The final temperature of the mixture was 37.73 °C. The final volume of water inside the calorimeter was 92.03 mL. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The volume of hot water added ml b. The mass of hot water (dwater = 1.00 g/mL) g...
1. A volume of water was heated to 83.90 °C and immediately added to 48.11 mL...
1. A volume of water was heated to 83.90 °C and immediately added to 48.11 mL of water at 23.98 °C contained within a coffee cup calorimeter. The final temperature of the mixture was 40.86 °C. The final volume of water inside the calorimeter was 90.45 mL. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The volume of hot water added ml b. The mass of hot water (dwater = 1.00 g/mL) c....
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water...
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water in a coffee cup calorimeter. The water was initially at 20.0°C and the final temperature of the resulting solution was recorded as 17.1°C. Calculate the experimental AHcoln (in units of kJ/mol NH.NO:) for the dissolution of NH NO3 (molar mass = 80.04 g/mol). Assume that no heat is lost to the calorimeter or the surroundings. The density of water is 1.00 g/mL and the...
A volume of water was heated to 82.86C and immediately added to 50.31 mL of water...
A volume of water was heated to 82.86C and immediately added to 50.31 mL of water at 22:45 °C contained within a coffee cup calorimeter. The final temperature of the mixture was 37,08°C. The final volume of water inside the calorimeter was 94.33 mL. Calculate the following: Note: Heat capacity a. volume of hot water added is 4.18 *Consider sig fig b. masses of hot and cold water (density of water = 1,00 g/mL) c. changes in temperature (AT) of...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HCl in a calorimeter. Both solutions were initially at 35.00°C and the final temperature of the resulting solution was recorded as 37.00°C. Write a balanced chemical reaction for the neutralization reaction between aqueous NaOH and HCl, determine the number of moles of water formed in this reaction, and calculate the overall heat change of the solution. Assume 1) that no heat is...
1) A calorimeter contains 28.0 mL of water at 11.5 ?C . When 2.20 g of...
1) A calorimeter contains 28.0 mL of water at 11.5 ?C . When 2.20 g of X (a substance with a molar mass of 51.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)?X(aq) and the temperature of the solution increases to 30.0 ?C . Calculate the enthalpy change, ?H, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g??C)], that density of water is...
A calorimeter contains 26.0 mL of water at 13.5 ∘C . When 2.50 g of X...
A calorimeter contains 26.0 mL of water at 13.5 ∘C . When 2.50 g of X (a substance with a molar mass of 51.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
A calorimeter contains 25.0 mL of water at 13.0 ∘C . When 2.40 g of X...
A calorimeter contains 25.0 mL of water at 13.0 ∘C . When 2.40 g of X (a substance with a molar mass of 64.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
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 ml'', specific heat capacity = 4.18 Jg'K')
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...
1. A volume of water was heated to 83.90 °C and immediately added to 48.11 mL of water at 23.98 °C contained within a coffee cup calorimeter. The final temperature of the mixture was 40.86 °C. The final volume of water inside the calorimeter was 90.45 mL. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The volume of hot water added ml b. The mass of hot water (dwater = 1.00 g/mL) c....
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water in a coffee cup calorimeter. The water was initially at 20.0°C and the final temperature of the resulting solution was recorded as 17.1°C. Calculate the experimental AHcoln (in units of kJ/mol NH.NO:) for the dissolution of NH NO3 (molar mass = 80.04 g/mol). Assume that no heat is lost to the calorimeter or the surroundings. The density of water is 1.00 g/mL and the...
A volume of water was heated to 82.86C and immediately added to 50.31 mL of water at 22:45 °C contained within a coffee cup calorimeter. The final temperature of the mixture was 37,08°C. The final volume of water inside the calorimeter was 94.33 mL. Calculate the following: Note: Heat capacity a. volume of hot water added is 4.18 *Consider sig fig b. masses of hot and cold water (density of water = 1,00 g/mL) c. changes in temperature (AT) of...
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