A coffee cup calorimeter is used to measure the heat of neutralization for this acid - base reaction. Hl(aq) + KOH(aq) -> Kl(aq) + H 2O(l) 40 mL of 0.325 M HI are reacted with 20.0 mL of 0.200 M KOH. Both solutions are initially at 20.500 degrees C. After the reaction has finished, the temperature of the mixture is 21.318 degrees C. The heat capacity of the calorimeter is 29.0 J/oC and the specific heat of the mixture is 4.184 J/goC. The density of the solution is 1.00 g/mL Calculate the Heat of neutralization for this reaction (kJ/mol) (Hint: KOH is the limiting reagent) ? = kj/mol

A coffee cup calorimeter is used to measure the heat of neutralization for this acid - base reaction. Hl(aq) + KOH(aq) -> Kl(aq) + H 2O(l) 40 mL of 0.325 M HI are reacted with 20.0 mL of 0.200 M KOH. Both solutions are initially at 20.500 degrees C. After the reaction has finished, the temperature of the mixture is 21.318 degrees C. The heat capacity of the calorimeter is 29.0 J/oC and the specific heat of the mixture is 4.184 J/goC. The density of the solution is 1.00 g/mL Calculate the Heat of neutralization for this reaction (kJ/mol) (Hint: KOH is the limiting reagent) ? = 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

When a 8.00 g8.00 g sample of KClKCl is dissolved in water in a calorimeter that has a total heat capacity of 3.77 kJ⋅K−1,3.77 kJ⋅K−1, the temperature decreases by 0.490 K.0.490 K. Calculate the molar heat of solution of KCl.
Determine how much energy in kJ is absorbed when 6.03 g of HA, the limiting reactant, are completely used in the reaction. 2 HA (s) + X(OH)2 (aq) --> XA₂ (aq) + 2 H₂O (g) AH = 647.7 kJ You may or may not need the following molar mass information: HA molar mass = 46.31 g/mol H F9 F10 F3 O D)) # 3 E D C F4 KAA णी व $ 4 R F F5 ➤ 11 V do in % 5 F6 T G A B A 6 F7 H F8 & 7 N 8 U J * 00 8 a M K €1 ( 9 O F11 Ö ) O F12 P PE
200.0 mL of 0.200 M HNO3 is added to 200.0 mL of 0.200 M KOH in a coffee cup calorimeter. The neutralization reaction that occurs can be described by the chemical equation- HNO3(aq) + KOH(aq) → KNO3(aq) + H₂O(l) Before the solutions are mixed they are both at 23.00 °C. After the mixing of the solutions the temperature increases until it remains constant at 24.39 °C. Assuming no heat lost to the surroundings, how much heat was lost in this reaction? (Assume the specific heats and densities of the solutions is the same as water.)
When a 3.00 g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity of 1.89 kJ · K¯¹, the temperature decreases by 0.210 K. Calculate the molar heat of solution of RbBr. AH S = soln kJ/mol
E In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH), was added to 70.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 23.98 °C to 28.07 °C. If the solution has the same density and BO 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 = kJ/mol H₂O
How do i combine these reactions for a combustion reaction?
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
When 4 grams of a certain compound is dissolved in 61 grams of water in a calorimeter, the temperature of the calorimeter changes from 25.00ºC to 26.98 ºC. Assuming that the specific heat capacity for the resulting solution is 4.184 J/(g oC), and the heat for this solvation is found as x kJ, what is the value of x?
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
You place 32.3 ml of 0.134 M Ba(OH), in a coffee-cup calorimeter at 25.00°C and add 60.6 ml of 0.433 M HCI, also at 25.00°C. After stirring, the final temperature is 28.63°C. {assume that the total volume is the sum of the individual volumes and that the final solution has the same density (1.00 g/ml) and specific heat capacity (4.184 J/g°C) as water}. Calculate the change in enthalpy, AH, of the reaction (in kJ/mol) of water formed. Enter the appropriate sign (+/-). Enter a number to 1 decimal place.
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.
A student followed the procedure in this experiment, using 29.5 mL of 1.66 molar HCl and 31.5 mL of 1.66 molar NaOH, with both solutions having an initial temperature of 22.1 oC. After mixing, a maximum temperature of 30.7 oC is measured. The final mass of the mixture was found to be 63.194 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format.