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Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 23.0 g...
Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 44.1 g...
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...
Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 25.9 g...
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...
A generic solid, X, has a molar mass of 61.6 g/mol. In a constant-pressure calorimeter, 18.3...
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?
A generic solid, X, has a molar mass of 72.6 g/mol. In a constant-pressure calorimeter, 16.6...
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...
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 74.3 g/mol. In a constant-pressure calorimeter, 11.5...
A generic solid, X, has a molar mass of 74.3 g/mol. In a constant-pressure calorimeter, 11.5 g of X is dissolved in 213 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 25.20 °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? = What is the enthalpy of the reaction? AH...
What mass of potassium nitrate (M = 101.1 g//mol) is required to prepare 300 mL of...
What mass of potassium nitrate (M = 101.1 g//mol) is required to prepare 300 mL of 0.1 M solution? b) What will be the concentration of potassium ions if extra 10 g of potassium sulfate (M = 174.3 g/mol) are added? Assume that the volume of the salt is negligible.
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...
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...
5.876 g of ammonium nitrate (M.W. 80.043 g/mol) was added to a calorimeter containing 99.270 g...
5.876 g of ammonium nitrate (M.W. 80.043 g/mol) was added to a calorimeter containing 99.270 g of water at 24.5 °C. After the NH4NO3 dissolved the final temperature reached was 20.0°C. Calculate 4sys for the dissolution of NH4NO3 The specific heat of water is 4.184 Jg-toc- and the heat capacity of the calorimeter (the "B" constant) is 15.0 J°C-.
5.876 g of ammonium nitrate (M.W. 80.043 g/mol) was added to a calorimeter containing 99.270 g...
5.876 g of ammonium nitrate (M.W. 80.043 g/mol) was added to a calorimeter containing 99.270 g of water at 24.5 °C. After the NH4NO3 dissolved the final temperature reached was 20.0 °C. Calculate sys for the dissolution of NH4NO3 The specific heat of water is 4.184 Jg-loc-1 and the heat capacity of the calorimeter (the "B" constant) is 15.0°C-1
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...
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 74.3 g/mol. In a constant-pressure calorimeter, 11.5 g of X is dissolved in 213 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 25.20 °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? = What is the enthalpy of the reaction? AH...
What mass of potassium nitrate (M = 101.1 g//mol) is required to prepare 300 mL of 0.1 M solution? b) What will be the concentration of potassium ions if extra 10 g of potassium sulfate (M = 174.3 g/mol) are added? Assume that the volume of the salt is negligible.
5.876 g of ammonium nitrate (M.W. 80.043 g/mol) was added to a calorimeter containing 99.270 g of water at 24.5 °C. After the NH4NO3 dissolved the final temperature reached was 20.0°C. Calculate 4sys for the dissolution of NH4NO3 The specific heat of water is 4.184 Jg-toc- and the heat capacity of the calorimeter (the "B" constant) is 15.0 J°C-.
5.876 g of ammonium nitrate (M.W. 80.043 g/mol) was added to a calorimeter containing 99.270 g of water at 24.5 °C. After the NH4NO3 dissolved the final temperature reached was 20.0 °C. Calculate sys for the dissolution of NH4NO3 The specific heat of water is 4.184 Jg-loc-1 and the heat capacity of the calorimeter (the "B" constant) is 15.0°C-1
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