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Assuming that the specific heat of the solution is 4.18 J/(g⋅∘C) and that the calorimeter itself...
Consider the combustion of propane: Assume that all of the heat comes from the combustion of propane (C_1H_8). Calculate DeltaH in which 5.00 g of propane is burned in excess oxygen at constant pressure. When 1.045 g of CaO is added to 50.0 mL of water at 25.0degreeC in a calorimeter, the temperature of the water increases to 32.3degreeC Assuming that the specific heat of solution is 4.18 J/(gdegreeC) and that the calorimeter itself absorbs a negligible amyl heat, calculate...
Question 7 of 16 > In a calorimeter, 1.045 g of an unknown salt is dissolved in 50.0 mL of water at 25.0 'C, and the temperature of the water increases to 32.3°C. Assuming that the specific heat of the solution is 4.184 J/g °C) and that the calorimeter itself absorbs a negligible amount of heat, calculate the AH in kJ for dissolving the salt in water. O 31.9 J -1.56 kJ 1.561 -1560 kJ O -31.9 O 1560 kJ...
A calorimeter contains 35.0 mL of water at 12.0 ∘C . When 2.30 g of X (a substance with a molar mass of 70.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 26.5 ∘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 calorimeter contains 27.0 mL of water at 14.0 ∘C . When 2.00 g of X (a substance with a molar mass of 77.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 26.5 ∘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 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...
A calorimeter contains 27.0 mL of water at 14.0 ∘C . When 2.00 g of X (a substance with a molar mass of 77.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 26.5 ∘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 calorimeter contains 24.0 mL of water at 13.0 ∘C . When 2.00 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 26.5 ∘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 calorimeter contains 18.0 mL of water at 13.0 ∘C . When 1.80 g of X (a substance with a molar mass of 82.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 27.5 ∘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...
Part A: A calorimeter contains 26.0 mL of water at 13.0 ∘C . When 2.10 g of X (a substance with a molar mass of 49.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘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...
Part A A calorimeter contains 34.0 mL of water at 12.5 ∘C . When 1.50 g of X (a substance with a molar mass of 75.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.5 ∘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...