*Ch.5 sect. 6 ~* Adding 4.379 ofthe SaltNH₁ NO 3 (S) +0 130g of water in a coffee-cupCalorimetry (with stirring to dissolveresulted17.1°C 10ina decrease in temperature from14,9 °CCalculate the enthalryChange for dissolving NH₂ NO₂ (s) in waterin K5/mol. Assume the solution (whose mass134. 4g) has a specific heat capacity ofis4.23/g.k(cold packs take advantages of thenitratefact that dissolvingisammoniuman endothermic Process)Enthalpy Changealt)A col pack uses the endothermic of asolutionof ammoniumnitrate.=- KJ/molin waterenthalpy6Iv.k

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* Adding 4.379 of NH₁ NO 3 (S) +0 13 Og of water in a coffee -cup Calorimetry (with stirring to dissolve resulted the salt) in a decrease in temperature from 17.1°C 10 14,9 °C. Calculate the enthalry. Change for dissolving NHM NO₂ (s) in water in kJ/mol. Assume the solution (whose mass is 134. 4g) has a specific heat capacity of 4.25/gk. (cold packs take advantages of the fact that dissolving ammonium nitrate is an endothermic Process). of ammonium A col Pack uses the endothermic enthalpy of a solution Enthalpy Change in water nitrate. jkJ/mol " v.k

* Adding 4.379 of NH₁ NO 3 (S) +0 13 Og of water in a coffee -cup Calorimetry (with stirring to dissolve resulted the salt) in a decrease in temperature from 17.1°C 10 14,9 °C. Calculate the enthalry. Change for dissolving NHM NO₂ (s) in water in kJ/mol. Assume the solution (whose mass is 134. 4g) has a specific heat capacity of 4.25/gk. (cold packs take advantages of the fact that dissolving ammonium nitrate is an endothermic Process). of ammonium A col Pack uses the endothermic enthalpy of a solution Enthalpy Change in water nitrate. jkJ/mol " v.k

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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2 A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.34 g of CoSO4(s) is dissolved in 101.00 g of water, the temperature of the solution increases from 25.00 to 26.69 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
A cubic piece of platinum metal (specific heat capacity = 0.1256 J/°C･g) at 200.0°C is dropped into 1.00 L of deuterium oxide ('heavy water,' specific heat capacity = 4.211 J/°C･g) at 25.5°C. The final temperature of the platinum and deuterium oxide mixture is 35.1°C. The density of platinum is 21.45 g/cm³ and the density of deuterium oxide is 1.11 g/mL. What is the edge length of the cube of platinum, in centimeters?
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In this experiment you will place a sample of your salt in water in a constant pressure calorimeter. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the number of moles of SrCl2? 4.368 g SrCl2 x ( 1 mol SrCl2 / 123.073 g SrCl2 ) = 0.035491131 mol SrCl2 a. 0.035491 mol SrCl2 b. none of these c. 0.035 mol SrCl2 d. 0.03 mol SrCl2 e. 0.0355 mol SrCl2 f. 0.04 mol SrCl2 g. 0.035491131 mol SrCl2 h. 0.03549 mol SrCl2
When a 13.3 g sample of NaOH(s) dissolves in 386.0 mL water in a coffee cup calorimeter, the temperature of the water changes from 22.5°C to 31.4°C. NaOH (8) — Na* (aq) + ОН (аq) Assuming that the specific heat capacity of the solution is the same as for water (4.184 J/g . °C) and the density of the solution is 1.031 g/mL, calculate the following. the heat transfer from system to surroundings (in J) a. b. AH for the reaction (in kJ) kJ
The combustion of 1.880 g of sucrose, C,H,,O, (s), in a bomb calorimeter with a heat capacity of 4.30 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.31 °C to 29.52 °C. What is the internal energy change, AU, for the combustion of 1.880 g of sucrose? AU = kJ Calculate the enthalpy of combustion, AHe, of sucrose in kilojoules per mole. kJ/mol AH. = A étv w MacBook Air DI DD 80 888 F12 F11 F9 F10 F7 FB 3 F4 F5 F6
When 34.5 mL of 0.545 M H2SO4 is added to 34.5 mL of 1.09 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate H of this reaction per mole of H2SO4 and KOH reacted. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water: d = 1.00 g/mL and c = 4.184 J/g×K.) H per mole of H2SO4 reacted: H per mole of KOH reacted:
10-A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.00°C and the temperature of the resulting solution was recorded as 37.00°C, determine the AH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HNO3. The specific heat capacity of water = 4.18 J/g°C. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water.
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.
A cubic piece of platinum metal (specific heat capacity = 0.1256 J/°C･g) at 200.0°C is dropped into 1.00 L of deuterium oxide ('heavy water,' specific heat capacity = 4.211 J/°C･g) at 25.5°C. The final temperature of the platinum and deuterium oxide mixture is 31.3°C. The density of platinum is 21.45 g/cm³ and the density of deuterium oxide is 1.11 g/mL. What is the edge length of the cube of platinum, in centimeters?
Adding 4.88 g of NH4NO3 (s) to 140 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 19.0 °C to 16.7 °C. Calculate the enthalpy change for dissolving NH4NO3 (s) in water in kJ/mol. Assume the solution (whose mass is 144.9 g) has a specific heat capacity of 4.2 J/g. K. (Cold packs take advantage of the fact that dissolving ammonium nitrate in water is an endothermic process.) ACE A cold pack uses the endothermic enthalpy of a solution of ammonium nitrate. Enthalpy change = esc A kJ/mol @2 2 W S #3 E D 20 F3 $ 4 888 F4 R F do LO % 5 Cengage Learning Cengage Technical Support T G MacBook Pro 6 F6 Y v lo 7 H 38 F7 U CO DII F8 F9 K F10 L P F11 { Save and Exit F12
A 3.450 g of propane (molar mass = 44.11 g/mol) was placed in a bomb calorimeter with excess oxygen and ignited. The initial temperature of the calorimeter was 24.000 degrees celsius and its total heat capacity was 76.65 kJ * C^-1. The reaction raised the temperature of the calorimeter to 28.965 degrees celsius. a. What is the heat exchangged by the reaction in kilojoules, qrxn? b. Calculate the deltaE rxn for the combustion of propane in kilojoules per mole c. Work in this reaction is done on the system, done on the surroundings, or equal to zero? Why?