If 7.5 g of KBr were dissolved in 100. g of water, how much heat (kJ) was involved? (2 Significant Figures) kJ J (q = msolution*C*AT where the heat capacity of the solution is 4.18
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Q: If 7.5 g of KBr were dissolved in 100. g of water, how much heat (kJ) was involved? (2 Significant…
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Q: Question 3
A: Given,Mass of barium chloride = 25gMass of water = 75gCalorimeter constant = 120J/degree Celsius.
Ti is 25C
I do not know what Tf is because I put 40 and it was wrong
Can you use this graph to help find Tf and use that to answer the equation
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- Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25C contains 15.0 mL of water at 25C. A 2.00-g sample of MgSO4 is dissolved in the water and 1.51 kJ of heat are evolved. (You can make the following assumptions about the solution: volume=15.0 mL, density=1.00 g/mL, specific heat=4.18J/gC.) (a) Write a balanced equation for the solution process. (b) Is the process exothermic? (c) What is qH2O? (d) What is the final temperature of the solution? (e) What are the initial and final temperatures in F?If 5.0125 g of calcium chloride (CaCl2) is dissolved in 100.0 mL of water, the following data are collected: starting temperature is 22.5 °C, final temperature is 27.9 °C. Calculate the enthalpy of solution (∆Hsolution) in Joules. You may assume a density of 1.00 g/mL for the solution and specific heat is 4.18 J/(g×°C). Given: q = - m · Cp · ∆T and ∆Hsolution =q/moles soluteWhen 1.3 g of KClO3 was added to 151.1 g of water in a calorimeter, the temperature dropped by 0.588 °C. The heat capacity of H2O is 4.184 J/g°C. Assume the specific heat of the solution equals that of pure H2O and that the calorimeter neither absorbs nor leaks heat. What is the molar heat of the solution of solid potassium chlorate? Give the answer in kJ, but do not include the unit
- A student determines the heat of dissolution of solid ammonium chloride using a coffee-cup calorimeter of negligible heat capacity.When 2.84 g of NH4Cl(s) is dissolved in 109.00 g of water, the temperature of the solution drops from 25.00 to 23.20 °C. Based on the student's observation, calculate the enthalpy of dissolution of NH4Cl(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.ΔHdissolution = kJ/molIf 5.0125 g of calcium chloride (CaCl2) is dissolved in 100.0 mL of water, the following data are collected: starting temperature is 22.5 °C, final temperature is 27.9 °C. Calculate the enthalpy of solution (∆Hsolution) in Joules. You may assume a density of 1.00 g/mL for the solution and specific heat is 4.18 J/(g×°C). Given: q = - m · Cp · ∆T and ∆Hsolution =q/moles solute a.) is it exothermic or endothermic and how do you know?Sodium chloride is added in cooking to enhance the flavor of food. When 10.0 g of NaCl is dissolved in 200.0 mL of water at 25.0 0 C I a coffee‐cup calorimeter. 669 J of heat are absorbed. (You can make the following assumptions about the solution. Volume = 200.0 mL, density is 1.0 g/mL, specific heat capacity = 4.18 J/g 0 C. a) Is the solution process endothermic? b) What is q H2O ? c) What is the final temperature of the solution?
- 80.0 mL of isopropanol (d = 0.825 g/cm3) initially at 5.00°C was added to 60.0 mL of ethanol (d = 0.795 g/cm3) initially at 27.5°C. If the specific heat of ethanol is 2.46 J/g. oC and the specific heat of isopropanol is 2.68 J/g. oC), what was the final temperature of the solution once the liquids were mixed?A student determines the heat of dissolution of solid cobalt(II) chloride using a coffee-cup calorimeter of negligible heat capacity.When 1.52 g of CoCl2(s) is dissolved in 117.00 g of water, the temperature of the solution increases from 25.00 to 27.00 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoCl2(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.ΔHdissolution = kJ/molMagnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25°C contains 15.0 mL of water at 25°C. A 2.00-g sample of MgSO4 is dissolved in the water and 1.51 kJ of heat are evolved. (You can make the following assumptions about the solution: volume = 15.0 mL, density = 1.00 g/mL, specific heat 5 4.18 J/g · °C.)(a) Write a balanced equation for the solution process.(b) What is qH2O?(c) What is the final temperature of the solution?
- Determine the final temperature of a 32.3 mL salt solution initially at 21.05ºC when 1.93 kJ of heat is added to the solution. The specific heat of the solution is 3.264 J/(ºC · g) and the density of the solution is 1.235 g/mL. Report your answer in units of degrees Celsius to 4 sig figs, but do NOT include units in your answer.A calorimeter initially contains 165.0 mL of water at 21.3oC. When 2.72 g K is added to the water, the temperature of the resulting solution rises to a maximum of 47.8oC. The reaction that occurs is:2K(s)+H2O(l)→2KOH(aq)+H2(g) Assuming no heat exchange between the calorimeter and the surroundings, calculate the heat of reaction, qreaction, in joules. (Use the total solution mass for the calculation, assume the density of water is 1.00 g/mL and the specific heat of the solution is 4.18 J/(g oC). J What is the enthalpy change, ΔH, in kilojoules per mole of K? kJ/mol K What is the enthalpy change for the reaction, ΔHreaction? kJ/molSodium chloride is added in cooking to enhance the flavor of food. V\lnen10.00 g of NaCl are dissolved in 200.0 mL of water at 25.0°C in a coffee cup calorimeter, 669 J of heat are absorbed. (You can make the following assumptions about the solution: volume = 200.0 mL, density = 1.00" g/mL, specific heat = 4.18J/g . °C)(a) Is the solution process exothermic?(b) What is qH2O?(c) What isthe finaltemperature of the solution?