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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When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 33.6 °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.
Macmillan Learning In a constant-pressure calorimeter, 55.0 mL of 0.300 M Ba(OH)₂ was added to 55.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 24.10 °C to 28.19 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C,) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = x10 TOOLS kJ/mol H₂O
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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
A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g.°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? q = kJ What is the enthalpy of the reaction? AHrxn 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.
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.
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.
When 3.50 g of sodium hydroxide (NaOH) was dissolved in 50.00 g of water a value of 9.50oC was obtained for ΔT. Calculate the value (calories) for the heat of solution of 3.50 g of NaOH. Calculate the number of calories that would be produced if one mole of sodium hydroxide was dissolved. (ΔHsolnNaOH)