The addition of 3.15 g ofBa(OH)2·8H2O to a solutionof 1.52 g of NHĄSCN in 100 g of water in acalorimeter caused the temperature to fall by 3.1 °C.Assuming the specific heat of the solution andproducts is 4.2O J/g°C, calculate the approximateamount of heat absorbed by the reaction, which canbe represented by the following equation:Ba(OH)2-8H,0 + 2NH,SCN Ba(SCN), + 2NH3 +10H,OO 136.28 J1.3628 JO 1362.8 J

Answered: Image /qna-images/answer/523647de-f3f5-4751-aed1-fac2bec3fb45.jpg

The addition of 3.15 g ofBa(OH)2•8H2O to a solution of 1.52 g of NH4SCN in 100 g of water in a calorimeter caused the temperature to fall by 3.1 °C. Assuming the specific heat of the solution and products is 4.20 J/g°C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)2-8H20 + 2NH,SCN Ba(SCN)2 + 2NH3 +10H;O O 136.28 J 1.3628 J O 1362.8 J

The addition of 3.15 g ofBa(OH)2•8H2O to a solution of 1.52 g of NH4SCN in 100 g of water in a calorimeter caused the temperature to fall by 3.1 °C. Assuming the specific heat of the solution and products is 4.20 J/g°C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)2-8H20 + 2NH,SCN Ba(SCN)2 + 2NH3 +10H;O O 136.28 J 1.3628 J O 1362.8 J

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...

See similar textbooks

Similar questions

During an experiment, a student adds 1.05 g of calcium metal to 200.0 mL of 0.75 M HCI. The student observes a temperature increase of 17.0 °C for the solution. Assuming the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the specific heat is 4.184 J/(g.°C), calculate the heat of the reaction, AHrxn - Ca(s) + 2 H*(aq) → Ca+(aq) + H, (g) %3D 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 =
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C. The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data. Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol). C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy
A 1.75 g sample of zinc metal is reacted with 128 g of 1.10 M hydrochloric acid solution in a constant-pressure calorimeter. The resulting solution changes in temperature from 22.58 °C to 22.97 °C. The hydrochloric acid is in excess. Based on this information, and estimating the solution's heat capacity as 4.18 Jg1 °C, what is the amount of heat, in joules, transferred in this reaction?
Determine the enthalpy of reaction (DHxn) in kJ/ mol H20 formed if an acid/base neutralization if 13.6 mL of 1.205 M NaOH is reacted with 25.0 mL of 1.108 M HCI causing an increase in the calorimeter temperature of 6.85 °C. Use 3.93 J/g°C for the specific heat capacity of the final solution and the density for the final solution is 1.02 g/mL.
A quantity of 2.00×102 mL of 0.786 M HCl is mixed with 2.00×102 mL of 0.393 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.76°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions? H+(aq) + OH−(aq)→H2O(l) _____°C
Solid calcium chloride dissolves in water according to the equation below.CaCl2 (s) ➝ Ca+2 (aq) + 2 Cl – (aq) ΔHº = –81.3 kJ/mol8.00 grams of solid CaCl2 dissolves in 45.0 grams of water initially at a temperature of 20.00 ºC in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g·ºC)]Tfinal = Answer ºC
Determine the change in enthalpy (H, in J) transferred when 8.0 g of sucrose (C12H22O11)are dissolved in 92.0 g of water in a coffee cup calorimeter. The temperature of the solution changesfrom 15.0 °C to 14.7 °C Assume the process takes place at constant pressure, the masses areadditive, and the specific heat of the solution is 4.18 J/g∙°C.
In an experiment, a 0.5002 g sample of tridecanedioic acid ( C13 H24 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.165 × 10³ g of water. During the combustion the temperature increases from 21.99 to 24.52 °C. The heat capacity of water is 4.184 J·g¯¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 904.0 J. °C¯¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of tridecanedioic acid based on these data. C13H24 O4(s) + 17O2 (g) → 12H₂O(l) + 13CO2 (g) + Energy kJ/mol Molar Heat of Combustion =
In a constant‑pressure calorimeter, 60.0 mL of 0.320 M Ba(OH)2 was added to 60.0 mL of 0.640 M HCl.The reaction caused the temperature of the solution to rise from 24.50 ∘C to 28.86 ∘C. If the solution has the same density and specific heat as water (1.00 g/mLand 4.184J/g⋅°C, respectively), what is ΔH for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes. ΔH= _________ kJ/mol H2O
Using the reaction enthalpy data shown, determine the amount of heat released in each situation: 2Ca (s) + O2 (g) ----> 2 CaO (s) ΔHrxn = -1,269.8 kJ a) if calcium reacts with 3.00 moles of O2 b) if 8.00 moles of calcium reacts with O2 c) if calcium and oxygen react to form 1.00 mole of CaO
A sample of NaOH (MM = 40.00 g/mol) with a mass of 1.811 g was added to a solution of HNO3 in a coffee cup calorimeter for a final volume of 100.0 mL. If both solutions were initially at 24.5 °C and the temperature of the resulting solution was recorded as 27.0 °C, determine the AH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH. Assume that the density and the heat capacity of the resulting solution are the same as water, 1.00 g/mL and 4.184 J/(g x °C) respectively. Your Answer: Answer units