In a constant-pressure calorimeter, 75.0 mL of 0.880 M H, SO, was added to 75.0 mlL of 0.440 M NaOH. The reaction caused the temperature of the solution to rise from 23.49 C to 26.49 C. If the solution has the same density and specific heat as water (1.00 g/ml. and 4.184 J/(g C), respectively), what is AH for this reaction (per mole of H,O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,0

In a constant-pressure calorimeter, 75.0 mL of 0.880 M H, SO, was added to 75.0 mlL of 0.440 M NaOH. The reaction caused the temperature of the solution to rise from 23.49 C to 26.49 C. If the solution has the same density and specific heat as water (1.00 g/ml. and 4.184 J/(g C), respectively), what is AH for this reaction (per mole of H,O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,0

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

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.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
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
Macmillan Learning In a constant-pressure calorimeter, 55.0 mL of 0.330 M Ba(OH), was added to 55.0 mL of 0.660 M HCI. The reaction caused the temperature of the solution to rise from 24.25 °C to 28.75 °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 = kJ/mol H₂O
48.2 mL of a solution of HCl is combined with 110.7 mL of 1.35 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C, and the final temperature after reaction is 29.3°C. What is the molarity of the HCl solution? You may assume that there is an excess of base (so that all the HCI has reacted), that the specific heat of the reaction mixture is 0.96 cal/g °C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mole.
When the Cacl2(s) is added to water, the following reaction occurs. Cacl (s) – Ca²"(aq) + 2CI"(aq) AH = - 81.5 kJ A 24.1 g sample of Caclz is dissolved in water, with both substances at 25.0 °C. Calculate the final temperature (in °C) of the solution assuming no heat is lost to the surroundings, the final solution, containing Cacl2 and water, has a mass of 100.0 g and the solution has a specific heat capacity of 4.18 J °c-lg-1. The molar mass of CaCl2 = 110.98 g/mol Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to one (1) decimal place. Answer: 59.0 The correct answer is: 67.3
In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH), was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 23.81 °C to 28.58 °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= kJ/mol H₂O
A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC. After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures. What is the heat transferred by this reaction, in Joules?
[11] A 10.00 g sample of a metal alloy was heated to 88.99 °C. It is then quickly dropped into 40.0 g of water in a calorimeter. The water temperature rises from 19.73 °C to 24.23 °C. Calculate the specific heat of the alloy. [Specific Heat of Water = 4.184 J/g °C and Heat Capacity of Calorimeter = 12.6 J/°C]
In a constant-pressure calorimeter, 65.0 mL of 0.910 M H₂SO, was added to 65.0 mL of 0.300 M NaOH. The reaction caused the temperature of the solution to rise from 24.00 °C to 26.04 *C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g °C), respectively), what is AH for this reaction (per mole of H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = V 5 R B 6 MacBook Air N 39 8 M command P option kJ/mol H₂O
How much heat is evolved when 8.89x10° g of ammonia is produced according to the following equation? (Assume that the reaction occurs at constant pressure.) N2(9) + 3H,(g) - 2NH3(g); AH = -91.8 k) kJ evolved
Payalben