You mix 125 mL of 0.320 M CSOH with 50.0 mL of 0.800 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 20.40 °C before mixing to 24.10 °C after the reaction. CsOH(aq) + HF (aq) → CsF(aq) + H₂O(l) What is the enthalpy of reaction per mole of CSOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g. K. Enthalpy of reaction = kJ/mol

You mix 125 mL of 0.320 M CSOH with 50.0 mL of 0.800 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 20.40 °C before mixing to 24.10 °C after the reaction. CsOH(aq) + HF (aq) → CsF(aq) + H₂O(l) What is the enthalpy of reaction per mole of CSOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g. K. Enthalpy of reaction = kJ/mol

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

Section 5.6 You place 0.0750 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCI. The reaction that occurs is: -> Mg (s) + 2 HCI (aq) → H2 (g) + MgCl2 (aq) The temperature of the solution raises from 20.15 °C to 23.29 °C. What is the enthalpy change or the reaction per mole of Mg? Assume that the specific heat capacity of the solution is 4.20 J/g K and the density of the solution is 1.00 g/mL. 412 kJ/mol 428 kJ/mol -412 kJ/mol -428 kJ/mol
A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
31. When a 0.740-g sample of trinitrotoluene (TNT), CH;N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter is 534 J C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?
A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol
When a 7.00 g sample of KCl is dissolved in water in a calorimeter that has a total heat capacity of 3.76 kJ⋅K−1, the temperature decreases by 0.430 K. Calculate the molar heat of the solution of KCl.
How much heat was absorbed by the solution? What is the enthalpy of the reaction?
Measurements show that the energy of a mixture of gaseous reactants decreases by 178. kJ during certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -163. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Round your answer to 2 significant digits. Is the reaction exothermic or endothermic? kJ exothermic endothermic x10 X
In a constant‑pressure calorimeter, 55.0 mL of 0.340 M Ba(OH)2 was added to 55.0 mL of 0.680 HCl. The reaction caused the temperature of the solution to rise from 23.90 ∘C to 28.53 ∘C. If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ).
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 323. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -162. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 significant digits. Is the reaction exothermic or endothermic? kJ exothermic O endothermic x10 X 3
In your Heat of Neutralization experiment, you will mix 25.0 mL of 1.0 M NAOH(ag) with 25.0 mL of 1.0 M HCI(ag) in a coffee-cup calorimeter; assume that you found the heat capacity of your calorimeter to be 25 J/°C. A graph of your data is shown below. What is the Heat of Neutralization in k] per mole? Neutralizaion Reaction of HCI(aq) and NaOH(aq) 30 8 26 AT 26 25 24 22 20 40 60 80 100 Time, s О а. -15 O b.-85 O C.-65 O d.-26 Temperature, oc
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl 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, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
When 0.376 g of sodium metal is added to an excess of hydrochloric acid, 3910 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCI(aq) 2 NaCl(aq) + H,(g) Enthalpy of reaction: 478.35 kJ Incorrect