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Calculate the final temperature when 30 mL of water at 75 °C are added to 65...
Part A Calculate the final temperature when 35 mL of water at 50 °C are added to 75 mL of water at 45 °C. Assume de...
Part A Calculate the final temperature when 35 mL of water at 50 °C are added to 75 mL of water at 45 °C. Assume density of water is 1.00 g/mL and no heat is lost to the calorimeter. IVO AQ o 2 ? Part A If the specific heat of methanol is 2.51 J/K-g, how many joules are necessary to raise the temperature of 12 g of methanol from 26°C to 78°C ? IVO AO + O 2 ?...
Calculate the final temperature when 90 mL of water at 85 °C are added to 10...
Calculate the final temperature when 90 mL of water at 85 °C are added to 10 mL of water at 20°C Assume density of water is 1.00 g/mL and no heat is lost to the calorimeter.
amount. 6. Calculate the final temperature when 50 mL of water at 65 °C are added to 25 mL of water at 25°C.
amount. 6. Calculate the final temperature when 50 mL of water at 65 °C are added to 25 mL of water at 25°C.
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...
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...
1a. A calorimeter contains 34.0 mL of water at 15.0 ∘C . When 2.40 g of...
1a. A calorimeter contains 34.0 mL of water at 15.0 ∘C . When 2.40 g of X (a substance with a molar mass of 62.0 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...
A calorimeter contains 35.0 mL of water at 14.5 ∘C . When 1.80 g of X...
A calorimeter contains 35.0 mL of water at 14.5 ∘C . When 1.80 g of X (a substance with a molar mass of 62.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 28.5 ∘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 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...
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...
Part A Calculate the final temperature when 35 mL of water at 50 °C are added to 75 mL of water at 45 °C. Assume density of water is 1.00 g/mL and no heat is lost to the calorimeter. IVO AQ o 2 ? Part A If the specific heat of methanol is 2.51 J/K-g, how many joules are necessary to raise the temperature of 12 g of methanol from 26°C to 78°C ? IVO AO + O 2 ?...
Calculate the final temperature when 90 mL of water at 85 °C are added to 10 mL of water at 20°C Assume density of water is 1.00 g/mL and no heat is lost to the calorimeter.
amount. 6. Calculate the final temperature when 50 mL of water at 65 °C are added to 25 mL of water at 25°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...
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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