When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (the following Figure), the temperature rises from 21.6°C to 37.8 °C. Review Constants (Figure 1) Part A Calculate AH (in kJ/mol NaOH) for the solution process NaOH (s) Na (aq) + OH (aq) Assume that the specific heat of the solution is the same as that of pure water. Figure < 1 of 1 Express your answer with the appropriate units. Thermometer ? Glass stirrer Value Units Cork stopper Submit Previous Answers Request Answer P Pearson s C Privacy Policy I Permissions / Contact Us Copyright © 2020 Pearson Education Inc. All rights reserved. | Terms of Use 100% ^ o search PrtSc F12 F11

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (the following Figure), the temperature rises from 21.6°C to 37.8 °C. Review Constants (Figure 1) Part A Calculate AH (in kJ/mol NaOH) for the solution process NaOH (s) Na (aq) + OH (aq) Assume that the specific heat of the solution is the same as that of pure water. Figure < 1 of 1 Express your answer with the appropriate units. Thermometer ? Glass stirrer Value Units Cork stopper Submit Previous Answers Request Answer P Pearson s C Privacy Policy I Permissions / Contact Us Copyright © 2020 Pearson Education Inc. All rights reserved. | Terms of Use 100% ^ o search PrtSc F12 F11

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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11.8 g of a soluble ionic compound is dissolved in 91.6 mL of water in a coffee-cup calorimeter, and the temperature of the solution changes from 24.80°C to 29.14°C. Assume the water has a density of 1.00 g/mL and that the total mass of the solution has the specific heat of water (4.186 J/g.K). Calculate the enthalpy change for the dissolution of this substance in kJ.
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When 17.98 g of calcium chloride (CaCl2) is dissolved in 681.87 g of water in a coffee-cup calorimeter at 26.4°C, the temperature increased to 28.4 °C. Assuming that the specific heat of the mixture is the same as the specific heat of pure water (4.184 J/g-°C), calculate the AH (in kJ/mol CaCl2) in the dissolution process. MW of CaCl2 = 110.9g/mol CaCl2 (s) →→ Ca+2 (aq) + 2 CI¯ (aq) Show your complete solution. Express your answer in two decimal places.
In a coffee cup calorimeter, 50.0 mL of 0.124 M AgNO3 and 50.0 mL of 0.124 M HBr are mixed. The following reaction occurs. Ag*(aq) + Br (aq) → AgBr(s) If the two solutions are initially at 23.92°C, and if the final temperature is 25.17°C, calculate AH for the reaction in kJ/mol of AgBr formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-1g-¹. kJ/mol
When 2.232 g of AX (s) dissolves in 147.5 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 34.8 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: · The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL · The liquid's final volume is not changed by adding the solid · The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.
Calculate the amount of salt in a commercial cold-pack containing ammonium nitrate (ΔHsol = + 25.7 kJ/mol) if the final temperature of the cold-pack is 3ºC. Assume that the initial temperature of water is 25ºC, mass of solution is 25 g and the specific heat of the solution is 4.184 J/g.K.
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 rnL of 1.00 M HCI are mixed. Both solutions were originally at 24.6 °C. After the reaction, the final temperature is 31.3 °C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s) + 2HCl(aq)-> ZnCl2(aq) + H2(g) When 0.115g of Zn(s) is combined with enough HCI to make 52.6mL of solution in a coffee - cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 21.5 °C to 24.7 °C. Part A Find \Delta Hrxn for this reaction as written. (Use 1.00 g/mL for the density of the solution and 4.18 J/(g°C) as the specific heat capacity.)
When a 7.41-g sample of solid potassium chlorate dissolves in 59.3 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 22.00 oC to 12.96 oC. Calculate H in kJ/mol KClO3 for the solution process. KClO3(s) K+(aq) + ClO3-(aq) The specific heat of water is 4.18 J/g-K.Hsolution = _________ kJ/mol KClO3.
How many grams of CaO must be added to 50.0 mL of water to make the temperature increase from 25.0 Â°C to 58.87 Â°C? The reaction is CaO(s) + H 2O(l) ↔ Ca(OH) 2(aq) -- ΔH = -83.7 kJAssume the heat capacity of the solution is the same as pure water (4.184 J/g*Â°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
A student determines the heat of dissolution of solid potassium bromide using a coffee-cup calorimeter of negligible heat capacity.When 4.93 g of KBr(s) is dissolved in 108.00 g of water, the temperature of the solution drops from 25.00 to 23.11 °C. Based on the student's observation, calculate the enthalpy of dissolution of KBr(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.ΔHdissolution = kJ/mol