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When 0.049 grams of a salt are dissolved in 45.3 grams of water in a calorimeter,...
When 10.0 grams of LiBr are dissolved in 100.0 grams of water in a calorimeter, the temperature increases from 30.00°C to 42.22°C. Use this information to determine the enthalpy change in units of kJ/mol of reaction. Assume the specific heat of the solution is the same as that of pure water (4.18 J/g •°C). -120. kJ -4.43 kJ -4.88 kJ -56.2 kJ -48.8 kJ
16) When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. The amount of heat absorbed by the water is _______J. (The specific heat of water is 4.18 J/g-°C.)
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...
When 16.3 g KOH is dissolved in 94.3 g of water in a coffee-cup calorimeter, the temperature rises from 18.9 °C to 30.16 °C. What is the enthalpy change per gram (in J/g) of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g×K. Water has a density of 1.00 g/ml. Be sure to enter the correct sign (+/-). Enter to 1 decimal place.
The salt sodium perchlorate is soluble in water. When 9.07 g of NaClO4 is dissolved in 103.00 g of water, the temperature of the solution decreases from 25.00 to 22.70 °C. Based on this observation, calculate the enthalpy of dissolution of NaClO4 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution kJ/mol =
Consider the dissolution of 1.50 grams of salt XY in 75.0 mL of water within a calorimeter. The temperature of the water decreased by 0.93 oC. The heat capacity of the calorimeter is 42.2 J/oC. The density of the water (and the solution) is 1.00 g/mL. The specific heat capacity of the solution is 4.184 J/goC. Identify the surroundings. Group of answer choices Salt dissolving in the water Calorimeter Water Solution and calorimeter
The salt cesium chloride is soluble in water. When 9.32 g CsCl is dissolved in 116,00 g water, the temperature of the solution decreases from 25.00 °C to 23.09 °C. Based on this observation, calculate the dissolution enthalpy, Adiss H. of CSCL Assume that the specific heat capacity of the solution is 4.184 J g'oc and that the energy transfer to the calorimeter is negligible. AdissH k J/mol Submit Show Approach Show Tutor Steps
The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00 g water, the temperature of the solution decreases from 25.00 °C to 22.56 °C. Based on this observation, calculate the dissolution enthalpy, ΔdissH, of CsCl. Assume that the specific heat capacity of the solution is 4.184 J g-1 °C-1 and that the energy transfer to the calorimeter is negligible. ΔdissH = kJ/mol
When 4.37 g of potassium bromide (KBr) is dissolved in 109 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 23.34 °C. Based on this observation, calculate q for the water and ΔH° for the process, assuming that the heat absorbed by the salt is negligible. KBr(s) --> K+(aq) + Br- (aq) The specific heat of water is 4.184 J °C-1 g-1.
Calorimetry A coffee cup calorimeter was used to measure the heat of solution - the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 130.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00°C to 23.70 °C. Calculate the enthalpy of solution, AH solution, per...