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A generic solid, X, has a molar mass of 74.3 g/mol. In a constant-pressure calorimeter, 11.5...
A generic solid, X, has a molar mass of 72.6 g/mol. In a constant-pressure calorimeter, 16.6 g of X is dissolved in 365 g of water at 23.00 °C. X($) — X(aq) The temperature of the resulting solution rises to 27.80 °C. Assume the solution has the same specific heat as water, 4.184 J/(g°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? 9 kJ What is the enthalpy of the...
A generic solid, X, has a molar mass of 61.0 g/mol. In a constant-pressure calorimeter, 25.5 g of X is dissolved in 387 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.00 °C. Assume the solution has the same specific heat as water, 4.184 1/(8°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? = KJ What is the enthalpy of the reaction?...
A generic solid, X, has a molar mass of 61.6 g/mol. In a constant-pressure calorimeter, 18.3 g of X is dissolved in 383 g of water at 23.00 °C.X(s) ͢ X(aq)The temperature of the resulting solution rises to 29.10 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there's negligible heat loss to the surroundings. How much heat was absorbed by the solution?What is the enthalpy of the reaction?
Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 23.0 g of KNO, is dissolved in 383 g of water at 23.00 °C. HO KNO,(s) + (aq) + NO3(aq) The temperature of the resulting solution decreases to 18.40 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g. "C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? Poln What is...
Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 25.9 g of KNO, is dissolved in 319 g of water at 23.00 °C. KNO,() K+(aq) + NO (aq) The temperature of the resulting solution decreases to 20.90 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g: "C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? What is the enthalpy...
Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 44.1 g of KNO3 is dissolved in 221 g of water at 23.00 °C. KNO3(s) to K+ (aq) + NO3- (aq) The temperature of the resulting solution decreases to 21.20 °C. Assume the resulting solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? How much heat was released...
A silver cube with an edge length of 2.25 cm and a gold cube with an edge length of 2.72 cm are both heated to 88.8C and placed in 101.5 mL of water at 19.6'C. What is the final temperature of the water when thermal equilibrium is reached? Substance gold silver water Specific heat (J/g.°C) 0.1256 0.2386 4.184 Density (g/cm) 19.3 10.5 1.00 Tonal 11 'C Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g)...
A calorimeter contains 19.0 mL of water at 11.5 ∘C . When 2.50 g of X (a substance with a molar mass of 63.0 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) 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 29.0 mL of water at 14.0 ∘C . When 1.30 g of X (a substance with a molar mass of 61.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 27.0 ∘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...