Dissolution is an endothermic process when 100 mL of water dissolves 5 grams ofa solid compound.Which direction does heat travel during the dissolution?a. From the system to the surroundingO b. From the surrounding to the systemC. Heat does not travel since both the system and the surrounding are at the same finaltemperaturesd. Heat does not travel since both the system and the surrounding are at the same initialtemperaturesP Type here to search

Dissolution is a endothermic process when 5g solid is dissolved into 100 ml of water. Direction of…

Answered: Dissolution is an endothermic process…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 7QAP: Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A...

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9.29 In which case is heat added to the system: (a) E=43J , w=40J ; or (b) E=31J , w=34J ?
Sodium chloride is added in cooking to enhance the flavor of food. When 10.00 g of NaCl are dissolved in 200.0 mL of water at 25.0C 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/gC) (a) Is the solution process exothermic? (b) What is qH2O? (c) What is the final temperature of the solution?
If the 3.21 g of NH4NO3 in Example 5.6 were dissolved in 100.0 g of water under the same conditions, how much would the temperature change? Explain your answer.
Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4 °C causes the temperature to rise to 25.8 °C. What is the approximate amount of heat involved in the dissolution, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?
If a substance has a positive enthalpy of solution, which would likely cause more of it to dissolve, hot solvent or cold solvent? Explain.
How does the process described in the previous item relate to the system shown in Figure 16.4?
Cooking A cook prepares a solution for boiling by adding12.5 g of NaCl to a pot holding 0.750 L of water. Atwhat temperature should the solution in the pot boil?Use Table 14.5 for needed data.
Magnesium sulfate (MgSO4) has a solubility of 38.9 g/ 100 g H2O at 30C. A solution is prepared by adding 9.50 g of MgSO4 to 25.0 g of water at 40C. A homogeneous mixture is obtained. Is the solution saturated, unsaturated, or supersaturated? One gram of magnesium sulfate is added to the solution cooled to 30C. Would you expect some of the MgSO4 to precipitate? If so, how much? If not, how much more MgSO4 can be added before precipitation takes place?
Dissolving 6.00 g CaCl2 in 300 mL of water causes the temperature of the solution to increase by 3.43 C. Assume that the specific heat of the solution is 4.18 J/g K and its mass is 306 g. (a) Calculate the enthalpy change when the CaCl2 dissolves. Is the process exothermic or endothermic? (b) Determine H on a molar basis for CaCl2(s)H2OCa2+(aq)+2Cl(aq)
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?
Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?
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.

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